This document provides a sample question paper for Chemistry (Class XII). It includes:
1. Details on the types of questions and their marks, totaling 70 marks.
2. The first few questions of the paper on topics like gas adsorption, noble gas species, and salt dissociation.
3. Instructions for the exam, including the time allowed and that calculators are not permitted.
Here are the answers to the practice questions:
1. Displacement reaction
2. (g) indicates the substance is in gaseous state
3. By storing in air tight containers to prevent reaction with oxygen
4. CO2 dissolves in water to form carbonic acid which reacts with calcium hydroxide to form calcium carbonate, making the solution milky
5. Nitrogen
6. By the direction of the gas bubbles - oxygen bubbles up and hydrogen bubbles down
7. Photodecomposition of hydrogen chloride to form hydrogen and chlorine
8. In the displacement reaction, iron displaces copper from its solution. The iron nail becomes coated with copper and the blue
Marking scheme-chemistry-perfect-score-module-form-4-set-4Mudzaffar Shah
The document provides a marking scheme for an exam on acids, bases, and salts. It includes:
1) 11 multiple choice questions on acid-base concepts like neutralization reactions, ions present, calculating molarity, and distinguishing between strong/weak acids.
2) 9 more multiple choice questions testing identification of solutions, gas tests, and acid/base properties.
3) 10 essay questions requiring explanations of acid/base definitions, calculations of standard solutions, titration procedures, comparisons of acid types, and writing hypotheses and procedures for experiments.
4) Rubrics for grading lab reports with criteria like correctly recording burette readings, setting up tables, stating observations/inferences, and comparing
This document contains a 33 question multiple choice chemistry test covering various topics in general, organic, and inorganic chemistry. The questions assess knowledge of atomic structure, chemical bonding, stoichiometry, acid-base chemistry, and the naming and properties of organic compounds including alkanes, alkenes, alcohols, ketones, aldehydes, carboxylic acids, esters, and amines.
This document is the cover page of a chemistry exam paper from the Malaysian Examinations Syndicate. It contains 50 multiple choice questions to be completed in 1 hour and 15 minutes. Students are instructed to choose only one answer for each question and mark their answers on the provided answer sheet. Calculators may be used. The questions cover topics in chemistry including the electron configuration of elements, chemical formulas, ionic compounds, acids and bases, the periodic table, chemical equations and reactions.
This tackles the basics and the easiest concept of Chemical reactions. This features only the four basic types of chemical reactions: synthesis, decomposition, metathesis, and ion - exchange reaction.
This is a basic concept because there is a pattern to be followed in each type of reaction.
More types of chemical reactions will be given on my next set of presentation entitled, "Everything You Want to Know About Chemical Reactions."
This document appears to be part of an exam for the Malaysian Certificate of Education (SPM) in Chemistry. It contains instructions for the exam, informing students that it will last 1 hour and 15 minutes and contains 50 multiple choice questions. It also provides some examples of chemistry questions and diagrams that may appear on the exam. The document provides context for a chemistry exam, but does not include any summaries on its own.
Question Analysis of Paper 1 Chemistry SPM 2013sweemoi khor
This document contains a table listing 50 chemistry questions from the 2013 SPM exam in Malaysia and their corresponding answers. The questions cover various chemistry topics including atomic structure, oxidation and reduction, manufacturing substances, carbon compounds, acids and bases, periodic table, chemical bonds, thermochemistry, and chemical formulas and equations. The answers range from A to D for each multiple choice question.
1. The document is an exam paper on acids and bases for IGCSE Chemistry. It contains 31 multiple choice questions testing knowledge of acid-base reactions and properties.
2. The questions cover topics like the characteristic properties of acids and bases, pH scales, acid-base indicators, and reactions like neutralization and those that produce carbon dioxide or ammonia gas.
3. Sample questions identify acids and bases, interpret acid-base titration curves, and write balanced equations for acid-base reactions.
This document contains a 30 question chemistry exam covering topics like:
- Properties and reactions of ionic/metallic substances
- Acid-base chemistry and nomenclature
- Thermochemistry and reaction kinetics
- Electrochemistry and metal extraction/refining methods
- Organic chemistry reactions, naming, and spectroscopy
The questions test understanding of concepts like conductivity, acidity, polymerization, enzyme catalysis, and require solving problems involving calculations with equations, concentrations, and thermodynamic quantities.
This document contains a 30 question chemistry exam covering various topics in chemistry including:
- Properties and reactions of ionic and metallic substances
- Coagulation processes and pyrometallurgy
- IUPAC naming of compounds
- Factors affecting melting points of carboxylic acids
- Relative reactivities and properties of white vs red phosphorus
- Relative basic strengths of amines
- Primary structural features of condensation polymerization
- Lead acid battery reactions
- Effect of temperature on reaction rates
- Principles of zone refining and van Arkel methods
- Properties of NF3 and bonds in SF4
- Balancing chemical equations
- Solubility properties of alcohols
This document provides information about chemistry questions and answers from a 2014 exam in Kedah, Malaysia. It includes the question paper for Module 2 Chemistry, with 50 multiple choice questions and answers. It also includes the mark scheme and answers for the paper. The document discusses the questions asked, the correct answers, and the number of marks awarded for each part of each question. It provides a detailed breakdown of the questions, expected answers and marking criteria for the chemistry exam.
Chemistry revision presentation on section b dan c past year paper = ogos 2011MRSMPC
The document describes two experiments on the reaction of zinc with acids P and Q. Both reactions produced zinc salts and hydrogen gas while increasing in temperature. Experiment I used hydrochloric acid and produced zinc chloride and hydrogen gas. The energy profile diagram shows the heat of reaction (ΔH), activation energies without and with a catalyst (E and E'), and explains the energy changes in the reaction.
Kertas 1 pep percubaan spm mrsm 2018 soalanNurAin949758
This document contains information about a chemistry exam, including:
- The exam is 1 hour and 15 minutes long and contains 34 printed pages and 2 blank pages.
- The exam paper is bilingual (English and Malay) and contains instructions for candidates.
- The exam contains multiple choice questions testing knowledge of chemistry concepts like the periodic table, oxidation, rates of reaction, electrolysis, indicators, and chemical equations.
The document describes a study on the use of pyridine 2,6-dicarboxylic acid to spectrophotometrically determine manganese (II) ions in aqueous solution. The metal ion forms a stable pink colored complex with the ligand at pH 1.5-2.5. The complex has maximum absorbance at 500 nm and a 1:1 metal-ligand ratio. Beer's law is obeyed for Mn(II) concentrations of 50-225 μg/mL. The method was used to determine Mn(II) in synthetic samples.
A student conducted an experiment using aluminium, iron, and copper metals and their sulfate salt solutions. Aluminium was found to be the most reactive metal as it displaced both iron and copper from their aqueous solutions. When barium chloride and sodium sulfate solutions were mixed, a white precipitate formed through a double displacement reaction. Heating lead nitrate produces yellow-brown lead oxide and brown nitrogen dioxide gas. Heating ferrous sulfate turns it from light green to brown and produces sulfurous oxide gas.
1) The document provides a chemistry exam for Class XII students with three sections - multiple choice questions, short answer questions, and descriptive answer questions.
2) The multiple choice section contains 16 questions testing concepts across the chemistry curriculum.
3) The short answer section contains 8 questions requiring students to provide explanations, equations, or names for various chemistry concepts.
4) The descriptive answer section provides 3 essay questions where students must explain processes, properties, or reactions in fuller detail. The exam aims to comprehensively test students' understanding of chemistry.
This document contains instructions and questions for a physics exam for Class XI. It is 3 pages long and has a total of 30 questions worth 70 marks. Questions 1-8 are 1 mark each, questions 9-18 are 2 marks each, questions 19-27 are 3 marks each, and questions 28-30 are 5 marks each. The exam covers topics in physics including motion, forces, work, energy, gravitation, properties of matter, heat and thermodynamics, oscillations and waves. Students are provided with relevant physical constants and formulas. They are not permitted to use calculators during the exam.
This document appears to be an examination for a Physics class covering various topics:
1) It contains 20 multi-part physics problems testing concepts like kinematics, forces, energy, momentum, properties of matter, heat, sound, and optics.
2) The problems cover the calculation of values like percentage error, rounding numbers, work, pressure, velocity, temperature changes, frequencies, trajectories, moments of inertia, Bernoulli's theorem, and fluid flow rates.
3) The document tests the student's understanding and ability to apply physics formulas to different scenarios and situations.
The document provides instructions for a 3-hour physics exam for Class 11 students. It contains 30 questions ranging from 1 to 5 marks each. The questions cover a range of physics topics including fundamental forces, motion, mechanics, heat, waves, and electricity. Students are informed that calculators are not permitted and various physical constants may be used. They are advised that all questions are compulsory and instructed on the internal choices provided in some questions.
The document is the instructions for a mathematics exam consisting of 3 sections (A, B, C) worth a total of 100 marks. Section A has 6 single-mark questions. Section B has 13 four-mark questions. Section C has 7 six-mark questions. Calculators are not permitted. Questions cover topics of relations, geometry, complex numbers, probability, and series.
The document is a physics examination paper containing 26 questions ranging from 2 to 5 marks each. It provides instructions for the exam, including the number and type of questions. The questions cover various topics in physics like units, motion, forces, energy, momentum, rotational motion, gravitation, and friction. Some questions ask students to derive equations, calculate numerical values, or explain concepts. The marking scheme at the end provides the expected answers and weightage for each question.
This document provides instructions and questions for a chemistry exam for CBSE Board Examination 2011-2012. It notes that the exam contains 30 questions ranging from very short answer to long answer. Students are instructed to write their code number and serial numbers for the questions. They are given 15 minutes to read the paper before the exam starts. The document provides general instructions about marking and the types of questions. It then lists 8 very short answer questions, 6 short answer questions and suggests completing 2 chemical equations as part of the exam.
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2. Multiple choice questions assess concepts like Iodoform test, reactivity of aldehydes vs ketones, oxidation of ketones vs aldehydes.
3. Short answer and long answer questions evaluate understanding of reactions like Cannizzaro reaction, Clemmensen reduction, distinguishing between structural isomers based on chemical tests.
Cbse class 12 chemistry sample paper 05 (for 2013)mycbseguide
This document contains a 30 question chemistry exam with questions ranging from 1 to 5 marks. It provides instructions on answering questions of different mark values and includes questions testing a range of chemistry concepts. Example questions ask about crystal structure, IUPAC naming, reaction mechanisms, equilibrium constants, colligative properties and organic synthesis.
1. The document contains questions related to chemistry concepts and reactions. It asks about the extraction of copper, placement of hydrogen in the periodic table, properties of hydrides, thermal stability of carbonates, redox reactions involving iron and chlorine, and acid-base reactions.
2. Multiple choice and structured questions are asked about definitions, distinguishing compounds, reaction mechanisms, and thermodynamic calculations using standard enthalpies of formation and combustion.
3. Questions cover topics like metallurgy, extraction of tin, partitioning, Hess's law, and distinguishing between coordination number, paramagnetism, and ligand strength. Relevant examples and equations are provided in the answers.
1 Question 1 (Alcohols and Carbonyl Compounds - 20 marks.docxjoyjonna282
1
Question 1 (Alcohols and Carbonyl Compounds - 20 marks)
(a) Why does hexan-2-one have a lower boiling point than hexan-2-ol?
O OH
(2)
(b) Dehydration of the compound below in acid gives mainly one product. Suggest, with a
reason, what would be the major product.
H
+
heatOH .
(1)
(c) Esters are known for their very pleasant fragrances. The aroma is dependent on the
starting materials used to prepare the ester. Give the original starting materials used to
produce the ester below.
O
O
(2)
(d) The substitution reaction between the alkyl halide below and water results in an alcohol.
2
(i) Show the full mechanism of the reaction as it occurs via an SN1 pathway. Identify
all the elements of the reaction.
(5)
(ii) Which factor can be investigated to determine if the reaction proceeds by a
unimolecular or bimolecular mechanism, and how is it relevant in terms of the
mechanism?
(2)
(iii) Explain briefly whether the chlorine analogue of the substrate would react faster
or slower than the given compound above.
(2)
(iv) Draw a fully labeled energy profile for this SN1 reaction.
(4)
3
Question 2 (Saccharides - Total 14 marks)
(a) Below is the Fischer projection of a sugar.
CHO
HHO
OHH
OHH
HHO
CH2OH
(i) Show a Haworth projection of the cyclic form of the sugar, identifying the
anomeric centre as either or .
(2)
(ii) Fully classify the saccharide above in terms of its optical rotation, carbon skeleton
and class.
(2)
(iii) When the compound is reduced with NaBH4, is the product optically active or
not? Explain your answer.
(2)
(b) What is the process called when the optical rotation of an aqueous solution of a pure
anomer of glucose changes with time? Use chemical structures to demonstrate what is
happening.
(3)
4
(c) The following question relates to the structure below:
A. B.
C.
O
HO
HO
OH
O
OH
O
HO
OH
O
HO
OH
O
O
HO2C
OH OH
(i) Use arrows to identify the glycoside links between sugars a and b as well as b and
c and name them appropriately.
(3)
(ii) Explain if this is a reducing sugar or not.
(2)
5
Question 3 (Amines and Amides - Total 11 marks)
(a) Briefly explain why amines have lower boiling points than amides of similar molecular
weight.
(2)
(b) (i) What is the name of the following amine?
N
(1)
(ii) What is the structure of 2,2-dimethylpentanamine?
(1)
(c) Give the outcome of the reactions below.
(i) Ph-NH2 + CH3-CO2H
(1)
(ii)
H3O
+
N
H
O
(2)
(d) The structure of N-methylpropanamide is given below.
N
H
O
Predict the solubility of N-methylpropanamide by showing the full extent of H-
bonding between the compound and water.
(2)
6
(e) Explain with refe ...
1. The document discusses sample papers for Class 12 Chemistry that are published by a private organization for student practice. It states that CBSE has not released these papers and is not related to them. (Section A)
2. It provides instructions for the sample paper, which has multiple choice, very short, short, and long answer questions worth varying marks. The paper covers topics like kinetics, equilibrium, redox, coordination chemistry etc. (Section B, C, D, E)
3. It clarifies that while the papers can be used for practice, the questions may not appear in the actual exam, and people should not spread rumors about question papers.
This document provides a sample chemistry exam paper with 30 questions testing various concepts in chemistry. The questions cover topics like stoichiometry, gas laws, electronic configuration, periodic properties, chemical bonding, thermodynamics, and organic chemistry. The paper tests knowledge through calculations, explaining concepts, deriving relationships, and predicting properties and reactions. It provides worked solutions for multiple choice and multi-part questions assessing a range of skills in chemistry.
F.Sc. Part 2 Chemistry Paper Rawalpindi Board 2008 (Malik Xufyan)Malik Xufyan
This document contains the questions from a chemistry exam for a student named Malik Xufyan. The exam has two parts - an objective multiple choice section with 17 questions worth 17 marks, and a subjective section with 33 questions worth 83 marks covering a range of chemistry topics. The subjective questions ask about properties of elements, organic chemistry reactions, inorganic compounds, industrial processes, and more. The document provides the context for a chemistry exam, but does not include any answers to the questions.
This document contains a chemistry document about coordination compounds with questions for practice. It includes:
- Very short answer (1 mark) questions testing definitions and names of coordination compounds.
- Short answer (2 mark) questions requiring explanations and examples of coordination compound concepts.
- Short answer (3 mark) questions requiring explanations, drawings of structures, and applications of coordination compounds using concepts like isomerism, crystal field theory and magnetic properties.
This document contains a 50-question multiple choice test on chemistry concepts. The questions cover topics like chemical formulas, periodic trends, chemical bonding, stoichiometry, acid-base reactions, and organic chemistry. Each question is followed by 4 answer choices labelled A, B, C, or D.
How do you account for the reducing behaviour of h3 po2 on the basis of its s...Bibek Chouhan
This document contains questions for a chemistry exam. It states that questions 1-10 are worth 1 mark each, questions 11-20 are worth 2 marks each, and question 21 is worth 5 marks. The questions cover various topics in chemistry including acids and bases, oxidation and reduction reactions, properties of elements and compounds, and preparation of chemicals.
This document provides information on surface chemistry concepts including adsorption, desorption, absorption, and sorption. It defines these terms and discusses the differences between adsorption and absorption. Factors that affect adsorption such as the nature of the adsorbent and adsorbate, pressure, temperature, and activation of the solid adsorbent are summarized. The document also discusses Freundlich adsorption isotherms, adsorption from solution, applications of adsorption, and concepts related to catalysis including activation energy and catalytic promoters and inhibitors.
This document discusses different types of solids and their properties. It begins by introducing the three states of matter and describing how atoms in solids are held together more strongly than in gases and liquids.
It then summarizes the two main types of solids - amorphous and crystalline. Amorphous solids like glass have irregular atomic arrangements while crystalline solids have orderly, repeating patterns. Crystalline solids can further be classified based on the bonding forces between their constituent particles as ionic, covalent, molecular or metallic. Each type of bonding gives rise to distinct physical properties.
The document also describes space lattices and unit cells, which are the repeating arrangements of atoms that define crystalline structure. There
1. The document discusses different types of defects that can occur in solid materials, including point defects, electronic imperfections, and stoichiometric and non-stoichiometric defects.
2. Point defects include vacancy defects like Schottky defects (cation and anion vacancies that preserve stoichiometry) and Frenkel defects (cation displacement to interstitial sites). Non-stoichiometric defects occur when the ratio of cations to anions changes.
3. Defects can lead to increased electrical conductivity as they provide free electrons and holes for charge transport. They also decrease crystal density and stability in some cases. Various defect types are common in different material classes like ionic crystals,
This document discusses amines, including their classification, preparation methods, physical and chemical properties, and reactions. Amines are derivatives of ammonia where hydrogen atoms are replaced by alkyl groups. They are prepared through reduction of nitro compounds, ammonolysis of alkyl halides, reduction of nitriles or amides, and other methods. Amines are basic due to the lone pair on the nitrogen. Primary and secondary amines are more basic than tertiary amines due to solvation effects. Aromatic amines are less basic than alkyl amines. Amines undergo reactions such as acylation, carbylamine formation, and electrophilic aromatic substitution.
K2Cr2O7 has the following key properties:
1. It forms orange crystals that melt at 669 K and are moderately soluble in cold water but less soluble in hot water.
2. It is a powerful oxidizing agent that oxidizes substances like I-, Fe2+, H2S, and SO2 in the presence of dilute sulfuric acid.
3. Its solutions change color from orange to yellow upon addition of an alkali due to the equilibrium between dichromate and chromate ions, and the color changes back to orange with an acid.
The document summarizes key points about d-block and f-block elements. It discusses the electronic configuration of transition metals and inner transition elements. It also provides information about the preparation of potassium dichromate and potassium permanganate. Some questions and answers related to the properties of transition metals and inner transition elements are also included.
Thermodynamics deals with energy changes in chemical reactions and their feasibility. It describes three types of systems - open, closed, and isolated - based on their ability to exchange energy and matter with surroundings. The first law of thermodynamics states that energy in an isolated system is constant and can neither be created nor destroyed. It is expressed as a change in internal energy (ΔU) of the system equals heat (q) absorbed plus work (w) done. Entropy is a measure of randomness or disorder in a system, which typically increases for spontaneous processes that are irreversible without external influence.
This document discusses key concepts in thermodynamics including:
1. It defines thermodynamics as dealing with energy changes in chemical reactions and their feasibility.
2. It describes open, closed, and isolated systems and different types of processes like isothermal, isobaric, isochoric, and adiabatic processes.
3. It explains important thermodynamic properties and concepts such as internal energy, enthalpy, Gibbs free energy, entropy, and the three laws of thermodynamics.
Biomolecules include carbohydrates, lipids, proteins, nucleic acids, and vitamins. Carbohydrates can be monosaccharides (such as glucose), oligosaccharides, or polysaccharides (such as starch and cellulose). Proteins are made of amino acids linked through peptide bonds. Important proteins include enzymes, antibodies, and hemoglobin. Nucleic acids such as DNA and RNA contain nucleotides and carry genetic information. Vitamins are organic compounds essential in small amounts for normal growth and activity.
1. Nitrogen does not form pentahalides due to the absence of d-orbitals to expand its valence beyond four.
2. NH3 has stronger intermolecular hydrogen bonding than PH3, giving it a higher boiling point.
3. NO2 dimerizes to pair up its odd electron and achieve octet configuration.
The document summarizes key information about group 16 elements (oxygen, sulfur, selenium, tellurium, and polonium) and their compounds. It describes their electronic configurations, physical properties like melting points and boiling points, oxidation states, and common compounds. It provides details on the preparation, properties, and reactions of important oxygen compounds like ozone, sulfur dioxide, and sulfuric acid. It also notes some anomalies of oxygen compared to other group 16 elements.
The document discusses the properties of group 15 (pnicogen) elements. It describes their electronic configurations, trends in atomic radius, ionization energy, electronegativity, and oxidation states down the group. It also discusses the anomalous properties of nitrogen, allotropes of phosphorus, properties of ammonia and phosphine, and reactions of nitric acid. Key reactions in the industrial production of ammonia and nitric acid are also outlined.
Medicines are chemical substances that treat diseases and reduce suffering from pain. They include analgesics like aspirin and narcotics like morphine for pain relief, tranquilizers for stress reduction, antiseptics for wounds, disinfectants, and antimicrobials like antibiotics and sulfa drugs. Antibiotics can be bactericidal, killing microbes, or bacteriostatic, stopping their growth. They come in broad-spectrum varieties effective against many bacteria or specific varieties. Other drug classes include antifertility drugs, antihistamines for allergies, and antacids for excess stomach acid. Food additives are added for preservation, flavor and color enhancement, and nutrition. These include artificial sweeten
This document contains a 30 question chemistry sample exam with multiple choice and long answer questions. It provides instructions for the exam, including question types and point values. The questions cover topics such as chemical formulas, hybrid orbitals, equilibrium reactions, acid-base chemistry, and organic chemistry reactions. Sample solutions are provided for some questions as examples. The exam is designed to test understanding of essential chemistry concepts and principles.
This document provides a chemistry sample paper with 30 questions covering various topics in chemistry. It includes very short answer questions (1 mark), short answer questions (2-3 marks) and long answer questions (5 marks). The questions test a range of concepts including stoichiometry, gas laws, equilibrium, electrochemistry, organic chemistry and more. Sample solutions are provided for some questions to illustrate the expected level of detail in the responses. The document serves as a practice test for students to evaluate their understanding of key chemistry concepts.
This document discusses several techniques for purifying organic compounds and determining their composition:
1) Crystallization separates impurities from a compound by dissolving it in a hot solvent and cooling to form pure crystals.
2) Sublimation separates compounds that sublime from non-subliming impurities by direct transition from solid to gas.
3) Chromatography separates mixtures based on differences in compounds' interactions with a stationary and mobile phase.
This document outlines the curriculum for Class XII chemistry in India. It includes 16 units covering topics in solid state, solutions, electrochemistry, chemical kinetics, and organic and inorganic chemistry. There are 160 periods for theory and 60 for practical work. The theory exam is 3 hours long and worth 70 marks. Practical exams evaluate volumetric analysis, salt analysis, experiments and project work out of 30 total marks. Key areas covered include chemical bonding, stoichiometry, equilibrium, redox reactions, organic compounds and biomolecules. The curriculum aims to develop students' understanding of fundamental chemical concepts through both classroom and hands-on laboratory instruction.
How to Configure Time Off Types in Odoo 17Celine George
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Front Desk Management in the Odoo 17 ERPCeline George
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we may assume that God created the cosmos to be his great temple, in which he rested after his creative work. Nevertheless, his special revelatory presence did not fill the entire earth yet, since it was his intention that his human vice-regent, whom he installed in the garden sanctuary, would extend worldwide the boundaries of that sanctuary and of God’s presence. Adam, of course, disobeyed this mandate, so that humanity no longer enjoyed God’s presence in the little localized garden. Consequently, the entire earth became infected with sin and idolatry in a way it had not been previously before the fall, while yet in its still imperfect newly created state. Therefore, the various expressions about God being unable to inhabit earthly structures are best understood, at least in part, by realizing that the old order and sanctuary have been tainted with sin and must be cleansed and recreated before God’s Shekinah presence, formerly limited to heaven and the holy of holies, can dwell universally throughout creation
The Jewish Trinity : Sabbath,Shekinah and Sanctuary 4.pdf
Chemistry sample paper 2014 15
1. Page 1 of 10
SAMPLE QUESTION PAPER
CHEMISTRY (043)
CLASS – XII – (2014-2015)
QUESTION PAPER DESIGN
CLASS XII CBSE
Types of Questions
S.No Type of Question Marks for
each
Question
No. of
Questions
Total Marks
1. Long Answers (LA) 5 03 15
2. Value based question 4 01 04
3. Short Answers-II(SA II) 3 12 36
4. Short Answers-I(SA I) 2 05 10
5. Very Short Answer (VSA) 1 05 05
Total 26 70
Type of questions VSA(1) SA1(2) SA2(3) VB(4) LA(5) Total(%)
Knowledge 2 1 1 - - 07 (10%)
Understanding - 2 4 - 1 21 (30%)
Application - 2 4 - 1 21 (30%)
HOTS (Higher order thinking skills) 2 - 1 - 1 10(14%)
Evaluation and Multi-disciplinary 1 - 2 1 - 11(16%)
2. Page 2 of 10
SAMPLE QUESTION PAPER
CHEMISTRY
CLASS – XII (2014 – 2015)
Time Allowed: 3 hr Maximum marks: 70
General Instructions:
(a) All questions are compulsory.
(b) Q.no. 1 to 5 are very short answer questions and carry 1 mark each.
(c) Q.no. 6 to 10 are short answer questions and carry 2 marks each.
(d) Q.no. 11 to 22 are also short answer questions and carry 3 marks each
(e) Q.no. 23 is a value based question and carry 4 marks.
(f) Q.no. 24 to 26 are long answer questions and carry 5 marks each
(g) Use log tables if necessary, use of calculators is not allowed.
1. The following figure shows the variation of adsorption of N2 on charcoal with pressure at
different constant temperatures:
3. Page 3 of 10
Arrange the temperatures T1, T2 and T3 in the increasing order.
2. Give the formula of a noble gas species which is isostructural with IBr2
-.
3. What is the effect of synergic bonding interactions in a metal carbonyl complex?
4. PCl5 acts as an oxidizing agent. Justify.
5. Write the name of the product formed when benzenediazonium chloride solution is treated with
potassium iodide.
6. Name the crystal defect which reduces the density of an ionic solid? What type of ionic
substances show this defect?
7. The molar conductivity (
m λ ) of KCl solutions at different concentrations at 298 K is plotted as
shown in the figure given below:
Determine the value of 0
m λ and A for KCl.
8. Aluminum crystallizes in anfcc structure. Atomic radius of the metal is 125 pm. What is the
length of the side of the unit cell of the metal?
9. Draw the structure of the following compounds:
(i) H2S2O7
(ii) XeOF4
OR
Write balanced chemical equations for the following:
(i) Reaction of chlorine with hot and concentrated NaOH.
4. (ii) Sulphur dioxide is passed through an aqueous solution of Fe (III) salt.
10. 0.5 g of KCl was dissolved in 100 g of water and the solution originally at 200C, froze at
-0.240C. Calculate the percentage dissociation of the salt.
(Given :Kf for water = 1.86 K kg /mol, Atomic mass: K = 39 u, Cl= 35.5 u)
11. State briefly the principles involved in the following operations in metallurgy. Give an
Page 4 of 10
example.
(i) Hydraulic washing.
(ii) Zone refining.
12.
i) What type of deviation from Raoult’s law is observed, when two volatile liquids A and
B on mixing produce a warm solution? Explain with the help of a well labeled vapour
pressure graph.
ii) Consider separate solutions of 0.5 M CH3OH, 0.250 M KCl (aq) and 0.125 M Na3PO4
(aq). Arrange the above solutions in the increasing order of their Van’t Hoff factor.
13. Write the Nernst equationand calculate the emffor the following cell at 298 K:
Mg(s) / Mg2+ (0.001 M) // Cu2+ (0.0001 M) / Cu(s)
How does Ecellvary with the concentration of both Mg2+ and Cu2+ ions?
(GivenEo
cell= 2.71 V)
14. Explain the following observations giving appropriate reasons:
(i) Ozone is thermodynamically unstable with respect to oxygen. .
(ii) The HEH bond angle of the hydrides of group 15 elements decrease as we move down
the group.
(iii) Bleaching effect of chlorine is permanent.
15.
(i) Predict the number of unpaired electrons in the tetrahedral [MnBr4]2- ion.
(ii) Draw structures of geometrical isomers of [Co(NH3)4Cl2]+.
(iii) Write the formula for the following coordinate compound:
Amminebromidochloridonitrito-N-platinate(II)
16. Explain what is observed when
(i) Silver nitrate solution is added to potassium iodide solution.
(ii) The size of the finest gold sol particles increases in the gold sol.
(iii) Two oppositely charged sols are mixed in almost equal proportions.
5. Page 5 of 10
17.
(i) In the following pairs of halogen compounds, which would undergo SN1 reaction
faster? Explain.
and
Cl
Cl
(ii) Amongst the isomeric dihalobenzenes which isomer has the highest melting point and
why?
(iii) Arrange the following haloalkanes in the increasing order of density. Justify your
answer.
CCl4, CH2Cl2 and CHCl3.
18. An organic compound ( A ) has characteristic odour. On treatment with NaOH, it forms
compounds ( B ) and ( C ). Compound ( B ) has molecular formula C7H 8Owhich on oxidation
gives back ( A ). The compound ( C ) is a sodium salt of an acid. When ( C ) is treated with
soda-lime, it yields an aromatic compound ( D ). Deduce the structures of ( A ), ( B ), ( C ) and
( D ). Write the sequence of reactions involved.
19. (a) Give one chemical test to distinguish between the following pairs of compounds:
(i) Methylamine and dimethylamine.
(ii) Aniline and benzylamine
(b) Write the structures of different isomers corresponding to the molecular formula C3H9N,
which will liberate nitrogen gas on treatment with nitrous acid.
20. (a) Exemplify the following reactions:
(i) Rosenmund reduction reaction.
(ii) Kolbe electrolysis reaction.
(b) Arrange the following compounds in increasing order of their reactivity towards HCN:
Acetaldehyde, Acetone, Di-tert-butyl ketone.
OR
(a) Predict the products of the following reactions:
6. Page 6 of 10
(i)
(i) Cl2 / Red phosphorous
(ii) H2O
CH3-CH2-COOH
(ii)
CH3
+ CrO2Cl2
(i) CS2
(ii) H3O+
(b) Arrange the following compounds in increasing order of acid strength:
Benzoic acid, 4-Nitrobenzoic acid, 4-Methoxybenzoic acid.
21.
(i) Identify the monomer in the following polymeric structure:
CN
[ CH2-CH=CH-CH2-CH2-CH ]n
(ii) On the basis of forces between their molecules in a polymer to which class does
neoprene belong?
(iii) Can both addition and condensation polymerization result in the formation of a co-polymer?
22.
(i) Which of the following biomolecule is insoluble in water? Justify.
Insulin, Haemoglobin, Keratin.
(ii) Draw the Haworth structure for α-D-Glucopyranose.
(iii) Write chemical reaction to show that glucose contains aldehyde as carbonyl group.
23. John had gone with his mother to the doctor as he was down with fever. He then went to the
chemist shop with his mother to purchase medicines prescribed by the doctor. There he
observed a young man pleading with the chemist to give him medicines as he had nasal
congestion. The chemist gave him cimetidine. John advised and also explained to the young
man that he should only take the medicines prescribed by the doctor.
Answer the following questions:
a) Did the chemist give an appropriate medicine? Justify your answer.
7. Page 7 of 10
b) John’s action was appreciated by his mother. List any two reasons.
24. (a) Write the mechanism of hydration of ethene to form ethanol.
(b) How are the following conversions carried out?
(i) Propanol to propan-2-ol.
(ii) Propanol to 1-propoxypropane.
(c) Give the structure and the IUPAC name of the major product obtained in the following
reaction:
OH
conc. HNO3
OR
(a) Write the mechanism of the reaction of HI with methoxymethane.
(b) Identify A and B in the following reactions:
(i)
OH
NaOH
A
(i) CO2
(ii) H+
B
(ii)
Cu, 573 K CH3MgBr
C2H5OH A B
H2O / H+
(c) Give the structure and the IUPAC name of the major product obtained in the following
reaction:
OC2H5 conc. HNO3
conc. H2SO4
25. (a) A blackish brown coloured solid (A) which is an oxide of manganese, when fused with
alkali metal hydroxide and an oxidizing agent like KNO3, produces a dark green coloured
8. compound (B). Compound (B) on disproportionation in neutral and acidic solution gives a
purple coloured compound (C). Identify A, B and C and write the reaction involved when
compound (C) is heated to 513 K.
(b)
(i) E0 M3+ / M2+values for the first series of transitionelements are given below.
Answer the question that follows:
E0 (V) Ti V Cr Mn Fe Co
M3+ / M2+ -0.37 -0.26 -0.41 +1.57 +0.77 +1.97
Identify the two strongest oxidizing agents in the aqueous solution from the
above data.
Page 8 of 10
ii) Copper (I) ion is not known in aqueous solution
iii) The highest oxidation state of a metal is exhibited in its oxide.
OR
(a) Write balanced equations to represent what happens when
(i) Cu2+ is treated with KI.
(ii) Acidified potassium dichromate solution is reacted with iron (II) solution.
(ionic equation)
(b)
i) The figure given below illustrates the first ionization enthalpies of first, second
and third series of transition elements. Answer the question that follows
9. Which series amongst the first, second and third series of transition elements have
the highest first ionization enthalpy and why?
ii) Separation of lanthanide elements is difficult. Explain.
iii) Sm2+, Eu2+ and Yb2+ ions in solutions are good reducing agents but an
aqueous solution of Ce4+ is a good oxidizing agent. Why?
Page 9 of 10
26.
i) Graphically explain the effect of temperature on the rate constant of reaction? How can
this temperature effect on rate constant be represented quantitatively?
ii) The decomposition of a hydrocarbon follows the equation
Calculate Ea
OR
i) In the reaction
Q + R → Products
The time taken for 99% reaction of Q is twice the time taken for 90% reaction of Q.
The concentration of R varies with time as shown in the figure below:
What is the overall order of the reaction? Give the units of the rate constant for the
same. Write the rate expression for the above reaction.
ii) Rate constant for a first order reaction has been found to be 2.54 x 10-3s-1.
Calculate its three-fourth life.
T
k x s e K (4.5 1011 1 ) 28000 = − −