Chemical Equilibrium Test

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Chemical Equilibrium Test - 8

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Question 1
1 / -0

The decomposition reaction, 4HNO₃(g) ⇌ 4NO₂ (g) + 2H₂O (g) + O₂ (g) is started with pure HNO₃ (g). If p is the tot al pressure at equilibrium, then

A

B

C

D

Solution
Question 2
1 / -0

For the equilibrium, SO₂ (g) + 1/2 O₂ (g) = SO₃ (g); ∆H = −99.0 kJ. The extent of forward reaction can be increased by

A
removing SO₃

B
using a catalyst

C
raising the temperature

D
lowering the pressure

Solution

Equilibrium shifts in the forward direction by removing SO₃ , decreasing the temperature and increasing the pressure. Catalyst does not disturb the equilibrium. Therefore, extent of forward reaction increases by removing SO₃ .
Question 3
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Consider the following reaction, and choose the correct option.

A
An increase in temperature will shift the equilibrium to the right, and so will an increase in pressure.

B
An increase in temperature and pressure will shift the equilibrium to the left.

C
An increase in temperature will shift the equilibrium to the left and on increase in pressure to the right.

D
Any increase in temperature and pressure will not shift the equilibrium.

Solution

The increase in temperature will favour the backward reaction, as the reaction is exothermic. With the increase of pressure on physical equilibria, the equilibrium will shift in that direction where the density is more. As the density of diamond is greater than graphite, thus increase in pressure will also favour backward reaction.
Question 4
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For the equilibrium,

which of the following statement is true?

A
The pressure changes do not affect the equilibrium.

B
More of ice melts, if pressure on the system is increased.

C
More of liquid freezes, if pressure on the system is increased.

D
The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system.

Solution

For heterogeneous physical equilibrium, with the increase of pressure, equilibrium shifts in the direction of physical state having higher density. This means that for the equilibrium, H₂O (s) ⇌ H₂O (I), more ice would melt on increasing the pressure of the system as density of water is more than ice.
Question 5
1 / -0

Ammonia gas at 76 cm Hg pressure was connected to a manometer. After sparking in the flask, ammonia partially dissociated as follows

The level in the mercury column of the manometer was found to show the difference of 18 cm. The partial pressure of H₂(g) at equilibrium is

A
18 cm of Hg

B
9 cm of Hg

C
24 cm of Hg

D
27 cm of Hg

Solution
Question 6
1 / -0

For the equilibrium A(g) + 2B(g) ⇌ AB₂ (g) the value of equilibrium constant at 300 k is 3 ×10^-3 mole^-2L² and value of equilibrium constant at 500 k is 5 ×10^-5 mole^-2L²

What is the sign of enthalpy change for this reaction

A
Positive

B
Negative

C
Data incomplete

D
Both (a) and (b) are possible at lower temperature it is positive and at high temperature it is negative.

Solution

Where, K₁ is equilibrium constant at temperature, T₁ and K₂ is equilibrium constant at temperature T₂ .

then, we can either substitute the values in equation and solve the problem or we can apply a simple mathematical logic and find the answer.

Alternately, You can remember this fact and apply it in questions directly. The fact is that the value of K_eq decreases on increase in temperature and vice-versa in case of exothermic reaction. The value of K_eq increases on increase in temperature in case of endothermic reaction.
Question 7
1 / -0

Following graph is plotted for the reaction:

2A (g) + B (g) ⇌ 2C (g)

In the graph the equilibrium state is reached at

A
t₁

B
t₂

C
t₃

D
t₄

Solution

At equilibrium, rate of forward reaction is equal to rate of backward reaction and at this situation concentration of each reactant and product becomes constant. Therefore, in graph-I at t₃ equilibrium is attained.
Question 8
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At –50°C, the self-ionization constant (ion product) of NH₃ is^K_^NH3 = 10^–30 M². How many amide ions are present per mm³ of pure liquid ammonia?

A
600 ions / mm³

B
6×10⁶ ions / mm³

C
6×10⁴ ions / mm³

D
60 ions / mm³

Solution
Question 9
1 / -0

The approach to the following equilibrium was observed kinetically from both directions.

At 25°C, it was found that

The value of K_c (equilibrium constant) for the complexation of the fourth Cl^– by Pt(II) is

A
53.8

B
50

C
60

D
63.8

Solution

At equilibrium, the rate of change of concentration of any species (reactant or product) is zero.

The equilibrium reaction for the complexation of the fourth Cl⁻ by Pt(II) is

Since, water is a solvent in the given reaction, so its concentration remains constant.

In the problem, expression of rate of change of concentration of is given, which at equilibrium is zero.
Question 10
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20 ml of O₂ contracts to 17 ml when subjected to silent electric discharge in an ozoniser. What is the volume of O₃ formed at equilibrium?

A
2 ml

B
8 ml

C
6 ml

D
4 ml

Solution

∴ x = 3

∴ Volume of O₃ formed = 2 × 3 = 6 ml