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11th Chemistry Monthly Test - 1 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Monthly Test - 1 ( Physical and Chemical Equilibrium )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

Which of the following is an example of homogeneous equilibrium?

H₂O(l) u21cc H₂O(g)
CaCO₃(s) u21cc CaO(s) + CO(g)
H₂(g) + I₂(g) u21cc 2HI(g)
2CO(g) u21cc CO₂(g) + C(s)

Hydrogen (a moles) and iodine (b moles) .react to give 2x moles of the HI at equilibrium. The total number of moles at equilibrium is

a+b+2x
(a-b)+(6-2x)
(a+b)
a+b-x

Consider the reaction CaCO₃(s) u21cc CaO(s) + CO₂(g) is a closed container at equilibrium. What would be the effect of addition of CaCO₃ on the equilibrium?

increases
remains unaffected
decreases
unpredictable

What is the correct expression for the representation of the solubility product constant of Ag₂CrO₄?

[Ag⁺]² [CrO₄²]
[2Ag⁺] [crO₄²]
[Ag⁺] [CrO₄^2-]
[2Ag⁺]² [crO₄²]

An equilibrium constant of 3.2 × 10^–6 for a reaction means, the equilibrium is

largely towards forward direction
largely towards reverse direction
never established
none of these

If x is the fraction of PCl₅ dissociated at equilibrium in the reaction
PCl₅ ⇌ PCl₃ + Cl₂
then starting with 0.5 mole of PCl₅, the total number of moles of reactants and products at equilibrium is

0.5 - x
x + 0.5
2x + 0.5
x + 1

The active mass of 7.0 g of nitrogen in a 2.0 L container would be

0.25
0.125
0.5
14.0

\(A+B\rightleftharpoons C+D,{ k }_{ c }\)for this reaction is 10. If c 1, 2, 3, 4 mole/litre of A, B, C and D respectively are present in a container at 25°C, the direction of reaction will be

From left to right
From right to left
Reaction is at equilibrium
Unpredictable

In the equilibrium reaction CaCO₃(s)u21cc CaO(s) + CO₂(g) whose concentration remains constant at a given temperature?

CaO
CO₂
CaCO₃
Both (a) and (c)

The value of AH for the reaction
\({ X }_{ 2\left( g \right) }+4Y_{ 2\left( g \right) }\rightleftharpoons 2XY_{ 4\left( g \right) }\) is less than zero. Formation of XY_4(g) will be favoured at :

High pressure and low temperature
Low pressure and low temperature
High temperature and high pressure
High temperature and low pressure.

Part - B

Generic 2 - Answer All Question

How is a gas-solution equilibrium exist?

(i)State Le-charteriers principle.
(ii )Write the complete thermochemical equation for the formation of NH₃ and mention which is endothermic & exothermic.

Ice melts slowly at higher altitudes. Explain why?

Distinguish between homogeneous and heterogeneous equilibrium reaction.

Write the expressions of equilibrium constants in terms of partial pressure and active masses for
\(2{ BrCl }_{ \left( g \right) }\rightleftharpoons { Br }_{ 2\left( g \right) }+{ Cl }_{ 2\left( g \right) }\)
Define the state of equilibrium.

When does the rate of backward reaction increase? What is its consequence?
\(A+B\rightleftharpoons C+D\)

The value of Kc for the reaction 2A u21c4 B + C is 2 x 10^-3. At a given time, the composition of
reaction mixture is [A] = [B] = [C] = 3 x 10^-4 M. In which direction the reaction will proceed?

When the numerical value of the reaction quotient (Q) is greater than the equilibrium constant (K), in which direction does the reaction proceed to reach equilibrium?

Write a balanced chemical equation for a equilibrium reaction for which the equilibrium constant is given by expression
\(K_c={[NH_3]^4[O_2]^5\over [NO]^4[H_2O]^6}\)

Part - C

Generic 3 - Answer All Question

At a certain temperature and total pressure of 10⁵Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I₂(g) u21cc 2I(g). Calculate K_p for the equilibrium

Given the equilibrium
N₂O₄(g) u21cc 2NO₂(g) with K_p = 0.15 atm at 298 K
(a) What is K, using pressure in torr?
(b) What is K_C using units of moles per litre.

Define melting point (or) freezing point of the substance.

Explain the effect of temperature on the following equilibrium reaction.
N₂(g) + 3H₂Cg)u21cc 2NH₃(g)Δ H = - 92.2 kJ.

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C
For the reaction
SrCO₃ (s) ⇌ SrO (s) + CO₂(g),
the value of equilibrium constant KP = 2.2 × 10^–4 at 1002 K. Calculate K_C for the reaction.

(i) Write a note on biochemical reversible change
(ii) State whether the existence of equilibrium is possible in our lungs or not. Give reason.

How does oxygen exchanges between maternal and fetal blood in a pregnant woman?

Write a note on Haber's process emphasizing the idea of effect of a catalyst in an equilibrium reaction.

What happens when the concentration of H₂ and I₂ are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

Part - D

Generic 5 - Answer All Question

1 mol of CH₄, 1 mole of CS₂ and 2 mol of H₂S are 2 mol of H₂ are mixed in a 500 ml flask. The equilibrium constant for the reaction K_C = 4 × 10^–2 mol² lit^–2. In which direction will the reaction proceed to reach equilibrium?

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

Derive the K_p and K_c for the following equilibrium reaction.
\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

Explain the effect of concentration, pressure, temperature, catalyst and inert gas on equilibrium.

The following water gas shift reaction is an important industrial process for the production of hydrogen gas.
CO(g) + H₂O(g) u21cc CO₂(g) + H₂(g)
At a given temperature K_p = 2.7. If 0.13 mol of CO, 0.56 mol of water, 0.78 mol of CO₂ and 0.28 mol of H₂ are introduced into a 2 L flask, and find out in which direction must the reaction proceed to reach equilibrium

The equilibrium constant for the following reaction is 0.15 at 298 K and 1 atm pressure.
N₂O₄(g) u21cc 2NO₂(g);
ΔHº = 57.32 KJmol^-1
The reaction conditions are altered as follows.
a) The reaction temperature is altered to 100o C keeping the pressure at 1 atm, Calculate the equilibrium constant.

Explain: How does the extent of reaction depend on K_c?
The equilibrium constant at 298 K for a reaction is 100.
A + B \(\rightleftharpoons \) C + D
If the initial concentration of all the four species is 1 M, the equilibrium concentration of D (in mol lit^-1) will be

1 mol of PCl₅, kept in a closed container of volume 1 dm³ and was allowed to attain equilibrium at 423 K. Calculate the equilibrium composition of reaction mixture. (The K_c value for PCl₅ dissociation at 423 K is 2)

At particular temperature K_C = 4 × 10^–2 for the reaction
H₂S(g) ⇌ H₂(g) + ½ S₂(g)
Calculate KC for each of the following reaction
i) 2H₂S (g) ⇌ 2H₂ (g) + S₂ (g)
ii) 3H₂S (g) ⇌ 3H₂ (g) + \(\frac{3}{2}\) S₂(g)

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