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CBSE Sample Paper for Class 11 Chemistry (Solved) – Set B
There is no overall choice in the paper. However, there is n internal choice in one question of 2 marks weight-age, one question of 3 marks weight-age and all t three questions of 5 marks weight age. Please note that the paper given here is only a sample. You can use log table if necessary. Use of calculator is not permitted. Set E of Solved CBSE Sample Paper for Class 11 Chemistry is given below with its solutions.
Sample Question Paper
1. The 4f subshell of an atom contains 10 electrons. What is the maximum number of electrons having spin in the same direction ? 
2. How is bond order related to bond length of a molecule ? 
3. What is the equation of state of an ideal gas for n moles ? 
4. Name a compound each in which the oxidation state of 0 is (i) + 2, and (ii) – 2. 
5. What happens when heavy water is added to calcium carbide ? 
6. How many grams of oxygen is required for complete combustion of 29 g of butane as per the equation :
C4H10 + 4.502 = 2CO2 + 5H2O 
7. Calculate the atomic mass (average) of chlorine using the following data : 
% Natural Abundance Molar Mass
35C1 75.77 34.9689
37C1 24.23 36.9659
8. One mole of H2O and one mole of CO are taken in a 10 litre vessel and heated at 725K. At equilibrium 40% of water (by mass) reacts with CO according to the equation :
H2O(g) + CO(g) → H2(g) + CO2(g)
Calculate the equilibrium constant for the reaction. 
9. What are pesticides ? Write any two pesticides. 
10. Which of the following compounds will show cis-trans isomerism ? 
(i) (H3C)2C = CH–C2H5
(ii) H2C = CBr2
(iii) C6H5CH = CHCH3
(iv) H3C—CH = CC1(CH3)
Why is Wurtz reaction not preferred for preparation of alkanes containing odd number of carbon atoms ?
Illustrate your answer by taking one example. 
11. A photon of wavelength 4 x 10-7 m strikes on metal surface, the work function of the metal being 2.13 eV. Calculate : (i) the energy of the photon (eV), (ii) the kinetic energy of the emission, and (Ai) the velocity of the photoelectron (1 eV = 1.602 x 10-19 J). 
12. In Rutherford’s experiment, generally thin-foils of heavy atoms like gold, platinum etc. have been used to be bombarded by the α-particles. If the thin foil of light atoms like aluminium etc. is used, what difference would be observed from the above results ? 
13. Discuss the shapes of the following molecules using the VSEPR model : 
BeC12, BC13, SiC14, AsF5 H2S, PH3
14. Complete and balance the following equation : 
Mn04– + H2S → Mn2+ + S (acidic medium)
15. Arrange the following : 
(i) CaH2, BeH2 and TiH2 in order of increasing electrical conductance.
LiH, NaH and CsH in order of increasing ionic character.
H—H, D—D and F—F in order of increasing bond dissociation enthalpy.
16. Cu+ and Na+ are of the same size but CuCl is insoluble in water while NaCl is soluble in water. Explain. 
17. What is the minimum volume of water required to dissolve 1 g of calcium sulphate at 298K? (for calcium sulphate, Ksp is 9.1 x 10-16) 
18. Pay load is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the pay load when a balloon of radius 10 m, mass 100 kg is filled with helium at 1.66 bar at 27°C. [Density of air = 1.2 kgm-3, R = 0.083 bar dm3K-1 mo1-1]. 
19. Have you ever observed any water pollution in your area ? What measures would you suggest to control it ? 
20. Complete the following reactions : 
21. (1) What do you mean by functional isomerism ?
(2) What is heterolytic cleavage ?
(3) What is inductive effect ? Give an example. 
22. State as to why : 
(a) a solution of Na2CO3 is alkaline ?
(b) alkali metals are prepared by electrolysis of their fused chlorides ?
(c) sodium is found to be more useful than potassium ?
Write balanced equations for the reactions between : 
(a) Na202 and water
(b) KO2 and water
(c) Na20 and CO2
23. A qualitative measure of the ability of an atom in a chemical compound to attract shared electrons to itself is called electronegativity. Unlike ionization enthalpy and electron gain enthalpy, it is not a measurable quantity. The electronegativity of any given, element is not constant; it varies depending on the element to which it is bound. Though it is not a measurable quantity, it does provide a means of predicting the nature of force that holds a pair of atoms together.
Now answer the following questions :
(i) What is the basic difference between the terms electron gain enthalpy and electronegativity ?
(ii) How would you react to the statement that the electronegativity of N on Pauling scale is 3.0 in all the nitrogen compounds ? 
24. Write expression for the work done by 1 mole of the gas in each of the following cases : 
(i) For irreversible expansion of the gas from volume V1 to V2.
(ii) For reversible isothermal expansion of the gas from volume V1 to V2.
(iii) For expansion of the gas into an evaluated vessel.
(iv) For reversible isothermal compression of the gas from pressure P1 to P2.
(v) For adiabatic expansion resulting into change of temperature from T1 to T2.
Justify the following statements : 
(a) Reactions with ΔG° < 0 always have an equilibrium constant greater than 1.
(b) Many thermodynamically feasible reactions do not occur under ordinary conditions.
(c) At low temperatures, enthalpy change dominates the AG expression and at high temperatures it is the entropy which dominates the value of ΔG
25. Discuss the chemistry of Lassaigne’s test. 
Describe the principle of estimation of phosphorus and oxygen in an organic compound. 
26. (a) Suggest a reason as to why CO is poisonous. 
(b) What do you understand by :
(a) inert pair effect, (b) allotropy, (c) catenation ? 
(a) In some of the reactions, thallium resembles aluminium, whereas in others it resembles with group I metals. Support this statement by giving some evidences. 
(b) When metal X is treated with sodium hydroxide, a white precipitate (A) is obtained, which is soluble in excess of NaOH to give soluble complex (B). Compound (A) is soluble in dilute HC1 to form compound (C). The compound (A) when heated strongly gives (D), which is used to extract metal. Identify (X), (A), (B), (C) and (D). Write suitable equations to support their identities.