Test 4 - Chemistry

Section A

1. Heat at constant volume and heat at constant pressure are, respectively:
1. $\Delta G ~~and ~~\Delta H $
2. $\Delta H ~~and ~~\Delta E $
3. $\Delta E ~~and ~~\Delta H $
4. $\Delta E ~~and ~~\Delta G $

2.

If a gas absorbs 200 J of heat and expands by 500 ${cm}^{3}$ against the constant pressure of 2x $10^{5}$ Nm^-2 , then the change in internal energy is :
1. $-$ 200 J
2. $-$ 100J
3. +100J
4. + 300J

3. The amount of heat required to raise the temperature of a body through 1 $^\circ C$ is called its:

1.	Molar Heat	2.	Specific Heat
3.	Entropy	4.	Heat capacity

4. If the equilibrium constant for a reaction $\mathrm{aA}+\mathrm{bB} \rightleftharpoons \mathrm{cC}+\mathrm{dD} \text { is } \mathrm{K}_c $ , then the equilibrium constant for the reaction $n a A+n b B \rightleftharpoons n c C+n dD $ will be equal to :
1. $n \sqrt {K_c} $
2. $\left(K_c\right)^n $
3. $\frac{K_c}{n} $
4. $n K_c $

5. The correct representation for the formation of CH₄(g) is:
1.  $\mathrm{C} (diamond )+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{4}(g)$
2.  $C(graphite) +4 \mathrm{H}{(g)} \longrightarrow \mathrm{CH}_{4}(g)$
3.  $\mathrm{C} (graphite) +2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{4}(g)$
4.  $C( diamond \left.)+4 \mathrm{H}{\mathrm{(g}}\right) \rightarrow \mathrm{CH}_{4}(g)$

6.

N₂ gas stored in a cylinder, fixed with a movable piston, undergoes adiabatic expansion. The statement that is true for the given situation is:
1. q=w
2. ∆U = w
3. ∆U=0
4. ∆U=q

7.

In the following, compressibility factor (Z) vs. pressure graph at 300 K, the compressibility of ${CH}_{4}$ at pressures<200 bar deviates from ideal behavior because

1.	The molar volume of CH₄ is less than its molar volume in the ideal state
2.	The molar volume of CH₄ is same as that in its ideal state
3.	Intermolecular interaction between CH₄ molecules decreases
4.	The molar volume of CH₄ is more than its molar volume in the ideal state

8. Select the correct graph/s for Boyle's law:

A.		B.
C.		D.

Choose the correct answer from the options given below:
1. C only
2. C and D only
3. A only
4. B and C only

9.

Which of the following reactions satisfies the condition $K_p>K_c \text { ? }$
1. H₂(g) + I₂(g) → 2HI(g)
2. N₂(g) + 3H₂(g) → 2NH₃(g)
3. 2SO₃(g) → 2SO₂(g) + O₂(g)
4. PCl₃(g) + Cl₂(g) → PCl₅(g)

10. Given below are two statements:

Statement I:	The expansion of gas against external pressure (P_ext $\neq$ 0) is called free expansion.
Statement II:	No work is done during the expansion of an ideal gas when the process is reversible only.

In light of the above statements choose the correct answer from the options given below:

1.	Both statement I and statement II are true.
2.	Both statement I and statement II are false.
3.	Statement I is correct but statement II is false.
4.	Statement I is incorrect but statement II is true.

11. Which of the following statements is true for a spontaneous process?

1.	The enthalpy change of the system must be negative.
2.	The entropy change of the system must be positive.
3.	The entropy change of the surroundings must be positive.
4.	The entropy change of the system plus its surroundings must be positive.

12. What is the density of N₂ gas at 227 °C and 5.00 atm pressure?
(R = 0.082 L Atm K^–1 mol^–1)
1. 1.40 g/L
2. 2.81 g/L
3. 3.41 g/L
4. 0.29 g/L

13. If the enthalpy of vaporization of $CCl_4$ is 15.4 kJ mol^-1, then the heat required for the vaporization of 30 g of $CCl_4$ at constant pressure is:
(Given: Molar mass of $CCl_4 = 154~ \text g~ \text {mol}^{-1}$)

1.	15.4 kJ	2.	3.0 kJ
3.	462 kJ	4.	5.13 kJ

14. A weak acid is titrated with a weak base. Consider the following statements regarding the pH of the solution at the equivalence point:

(i)	pH depends on the concentration of acid and base.
(ii)	pH is independent of the concentration of acid and base.
(iii)	pH depends on pK_a of acid and pK_b of base.
(iv)	pH is independent of pK_a of acid and pK_b of base.

The correct statements are :

1.	only (i) and (iii)	2.	only (i) and (iv)
3.	only (ii) and (iii)	4.	only (ii) and (iv)

15. Consider the Maxwell-Boltzmann distribution curve for a gas at the temperatures, T₁, T₂ and T₃ shown below:

The correct relationship between T₁, T₂ and T₃ is:
1. T₁ > T₂ > T₃
2. T₃ > T₂ > T₁
3. T₁ = T₂ = T₃
4. T₃ > T₁ > T₂

16.

$3 \mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{O}_{3}(\mathrm{g}) $
For the above reaction at 298 K, $\text K_c$ is found to be $3.0 \times 10^{-59} $. If the concentration of $\text O_2$ at equilibrium is 0.040 M, then the concentration of $\text O_3 $ in M is:
1. $1.2 \times 10^{21} $
2. $4.38 \times 10^{-32} $
3. $1.9 \times 10^{-63} $
4. $2.4 \times 10^{31} $

17.

When equal volumes of the following solutions are mixed, in which case will AgCl (K_sp= 1.8×10^–10) precipitate?
1. 10^–4M Ag⁺ and 10^–4M Cl^–
2. 10^–5 M Ag⁺ and 10^–5 M Cl^–
3. 10^–6 M Ag⁺ and 10^–6 M Cl^–
4. 10^–10 M Ag⁺ and 10^–10 M Cl^–

18.

The value of K_c for the reaction 2A $⇋$ B + C is 2 × 10^–3. At a given time, the composition of the reaction mixture is [A] = [B] = [C] = 3 × 10^–⁴ M.
The reaction will proceed:
1. In the backward direction
2. In the forward direction
3. In both direction
4. Cannot be predicted

19.

For the reaction, 2SO_2(g) + O_2(g) = 2SO_3(g), $∆$ H = –57.2 kJ mol^–1 and K_C= 1.7 × 10¹⁶ .
Which of the following statements is incorrect?

1.	The equilibrium will shift in the forward direction as the pressure increases.
2.	The addition of inert gas at constant volume will not affect the equilibrium constant.
3.	The equilibrium constant is large suggestive of the reaction going to completion and so no catalyst is required.
4.	The equilibrium constant decreases as the temperature increases.

20.

The oxidation states of phosphorous in H₃PO₃, P₄ and PH₃ respectively are:
1. +3, zero and -3
2. -3, zero and +3
3. +3, +4 and -3
4. +3, zero and +3

21. Given below are two statements:

Assertion (A):	The addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl.
Reason (R):	K_spof AgCl < K_spof AgBr

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

22.

Which one of the following is true for any diprotic acid, H₂X?
1. K_a2 = K_a1
2. K_a1 > K_a2
3. K_a1 < K_a2
4. $K_{a1}=\frac{1}{K_{a2}}$

23. In given reactions, mark option in which the underlined species acting as an oxidizing agent among the following:
1. Cl₂ + 2KBr → 2KCl +Br₂
2. Zn + CuSO₄ → ZnSO₄ + Cu
3. 3CO + Fe₂O₃ → 3CO₂ + 2Fe
4. H₂SO₄+ 2NaOH → Na₂SO₄ + 2H₂O

24. The strongest conjugate base is
1.  $Cl^-$
2.  $NO^-_3$
3.  $HCO^-_3$
4. $HSO^-_4$

25.

Assertion (A):	For an exothermic reaction, the value of K_cdecreases on increasing the temperature.
Reason (R):	Rate constant for a backward reaction increases more than the increase in the rate constant for a forward reaction.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are False.

26. The packing efficiency in case of simple cubic unit cell is:
1. ${2 \pi \over 3}$
2. ${ \pi \over 3}$
3. ${\pi \over 4}$
4. ${\pi \over 6}$

27. 651 g of ethylene glycol (HOCH₂CH₂OH) (M.W =62.1 g/mol) is dissolved in 1.5 kg of water at 363 K. The vapour pressure of pure water at 363 K is 0.7 atm. Assuming ideal solution behaviour, the vapour pressure of water over the solution (in atm) is closest to:
1. 0.57
2. 0.62
3. 0.65
4. 0.68

28. When an electrolytic solution is diluted, then the incorrect statement from the following is:
1. Specific conductivity increases
2. Molar conductivity increases
3. Equivalent conductivity increases
4. Specific conductivity decreases

29. The standard reduction potential of Zn²⁺/Zn and Cu²⁺/Cu is -0.76 and +0.34 V respectively. The oxidising agent and reducing agent, respectively, are

1.	Cu & Zn²⁺	2.	Zn & Cu
3.	Cu²⁺& Zn²⁺	4.	Cu²⁺& Zn

30. On dissolving urea in 500 g of water and cooling up to 272.65 K, 128 g of ice separates out of the solution. The amount of dissolved urea is :
$(K_f = 1.86 \ K ~ \text {kg} / \text {mol}) $
1. 0.06 g
2. 0.6 g
3. 6.0 g
4. 60 g

31. K_H value for some gases at the same temperature 'T' are given:

gas	K_H/k bar
Ar	40.3
CO₂	1.67
HCHO	1.83 × 10^–5
CH₄	0.413

K_H is Henry's Law constant in water. The order of their solubility in water is :

1.	Ar < CO₂ < CH₄ < HCHO
2.	Ar < CH₄ < CO₂ < HCHO
3.	HCHO < CO₂ < CH₄ < Ar
4.	HCHO < CH₄ < CO₂ < Ar

32.

Match Column-I (Types of cell) with Column-II (Characteristics shown by cells) and mark the appropriate option:

Column I (Type of cell)		Column II (Characteristics)
A	Lechlanche cell	1.	Cell reaction 2H₂ +O₂ → 2H₂O
B	Ni-Cd cell	2.	Does not involve any ion in solution and is used in hearing aids.
C	Fuel cell	3.	Rechargeable
D	Mercury cell	4.	-Reaction at anode, Zn → Zn²⁺ + 2e^-

Codes:

Options:	A	B	C	D
1.	2	3	4	1
2.	4	3	1	2
3.	1	4	3	2
4.	4	1	3	2

33. The crystal structure of white tin is:
1. Tetragonal
2. Cubic
3. Hexagonal
4. Orthorhombic

34. 40 cm³of a solution of sodium hydroxide is exactly neutralized by 25 cm³ of 0.40 mol L^–1 sulphuric acid.
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O
What is the concentration, in g L^–1, of the sodium hydroxide solution?
[Molecular mass value: NaOH = 40]
1. 20 gL^-1
2. 5 gL^-1
3. 0.25 gL^-1
4. 10 gL^-1

35. The amount of $\text{CaCl}_2~ (i = 2.47) $ that must be dissolved in 3 litre of water such that its osmotic pressure is 4.94 atm at 27 °C is:
1. $2.405 \times 10^{-3} ~ \text {mol} $
2. $0.243 ~ \text {mol} $
3. $0.0267 ~ \text {mol} $
4. $1.486 ~ \text {mol} $

Section B

36.

In a conductance cell containing a $0.1 \text { M KCl}$ solution, the resistance measured is $300 \text { ohm}$. The conductivity of the solution is given as $0.013 ~\mathrm{ S cm^{-1}} $. What is the cell constant of this conductance cell?
1. $\text{0.39}~\mathrm{ cm^{-1}} $
2. $\text{39}~\mathrm{ cm^{-1}} $
3. $\text{3.9}~\mathrm{ cm^{-1}} $
4. None of the above

37. Select the correct option based on statements below:

Assertion (A):	In a particular point defect, an ionic solid is electrically neutral, even if few of its cations are missing from its unit cells.
Reason (R):	In an ionic solid, Frenkel defect arises due to dislocation of cation from its lattice site to interstitial site, maintaining overall electrical neutrality.

1.	(A) is false but (R) is true.
2.	Both (A) and (R) are true and (R) is the correct explanation of (A).
3.	Both (A) and (R) are true but (R) is not the correct explanation of (A).
4.	(A) is true but (R) is false.

38. What fraction of Fe exists as Fe(III) in Fe_0.96O?
(Consider Fe_0.96 to be made up of Fe(II) and Fe(III) only)
1. $\dfrac{1}{12}$
2. $0.08$
3. $\dfrac{1}{16}$
4. $\dfrac{1}{20}$

39.

Assertion (A):	$E^0_{cell}$ is negative for electrolytic cell.
Reason (R):	$\Delta G $º is +ve for electrolytic cell.

1.	Both (A) and (R) are true and (R) is the correct explanation of (A).
2.	Both (A) and (R) are true but (R) is not the correct explanation of (A).
3.	(A) is true but (R) is false.
4.	(A) is false but (R) is true.

40. What is the Van't Hoff factor (i) for Al₂(SO₄)₃ if it dissociates to 40%?

1.	2.0	2.	2.6
3.	3.6	4.	5.0

41. When 2 faradays of electricity is passed through $AlCl_3$ solution, then the weight of aluminium deposited will be:
1. 27 gram
2. 18 gram
3. 9 gram
4. 54 gram

42. The INCORRECT statement about the conductivity of electrolytic (ionic) solutions is:

1.	It is independent of the solvent viscosity
2.	It depends on the size of the ions and their solvation
3.	It increases with the increase in electrolyte concentration
4.	It increases with the increase in temperature

43.

For a first-order reaction A $\rightarrow$ Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min^-1 is

1.	0.2303	2.	1.3818
3.	0.9212	4.	0.4606

44.

Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:
1. L mol^–1 s^–1
2. no unit
3. mol L^–1s^–1
4. s^–1

45.

Statement I:	$\Delta H $ of adsorption is always negative.
Statement II:	$\Delta S $ of adsorption is negative.

1.	Statement I is incorrect and statement II is correct
2.	Statement I is correct and statement II is incorrect
3.	Both statements I and II are correct
4.	Both statements I and II are incorrect

46. Consider the following reaction:
$A(g) \rightarrow B(g) + C (g)~$
The initial pressure is$P^o$ and the pressure at 't' time is$P_t (P_t>P^o)$. Assuming that the above reaction is of first order, the rate expression will be:
1. $K = {2.303 \over t}log {P^o \over P_t}$
2. $K = {2.303 \over t}log {2P^o \over P^o - P_t}$
3. $K = {2.303 \over t}log {P^o \over 2P^o - P_t}$
4. $K = {2.303 \over t}log {2P^o \over 3P^o- P_t}$

47.

The rate constant for a chemical reaction that takes place at 500 K is expressed as K = A e^-1000. The activation energy of the reaction will be:
1. 100 cal/mol
2. 1000 kcal/mol
3. 10⁴ kcal/mol
4. 10⁶ kcal/mol

48. The process of removing ions (or molecules) from a sol by diffusion through a permeable membrane is called:

1. Ultrafiltration
2. Dialysis
3. Electrophoresis
4. Osmosis

49. Thermal decomposition of N₂O₅ occurs as per the equation below:
2 N₂O₅ → 4 NO₂ + O₂
The correct statement is:

1.	Production rate of O₂ is four times the production rate of NO₂.
2.	Production rate of O₂ is the same as the rate of disappearance of N₂O₅.
3.	Rate of disappearance of N₂O₅is one-fourth of the production rate of NO₂.
4.	Rate of disappearance of N₂O₅is twice the rate of production of O₂.

50. The correct graph for the Arrhenius equation is:

1.		2.
3.		4.

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Assertion (A):	\(E^0_{cell}\) is negative for electrolytic cell.
Reason (R):	\(\Delta G \)º is +ve for electrolytic cell.

Statement I:	\(\Delta H \) of adsorption is always negative.
Statement II:	\(\Delta S \) of adsorption is negative.

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