Chemical Equilibrium Test

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Chemical Equilibrium Test - 4

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Weekly Quiz Competition

Question 1
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Which of the following is not a general characteristic of equilibria involving physical processes?

A
Equilibrium is possible only in a closed system at a given temperature.

B
All measurable properties of the system remain constant.

C
All the physical processes stop at equilibrium.

D
The opposing processes occur at the same rate and there is a dynamic but stable condition.

Solution

The physical processes do not stop at equilibrium. There is a state of dynamic equilibrium in these processes.
Question 2
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Which of the following conditions represent(s) an equilibrium?

A
Freezing of ice in a open vessel, where the temperature of ice is constant.

B
A few drops of water are present along with air in a balloon, where the temperature of the balloon is constant.

C
Water is boiling in an open vessel over stove, where the temperature of water is constant.

D
All of these

Solution

Equilibrium can be achieved only in closed vessel (the balloon in this case).
Question 3
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Which of the following statements is incorrect?

A
In an equilibrium mixture of ice and water kept in a perfectly insulated flask, the masses of ice and water do not change with time.

B
The intensity of red colour increases when oxalic acid is added to a solution containing iron (III) nitrate and potassium thiocyanate.

C
On addition of catalyst, the equilibrium constant value is not affected.

D
Equilibrium constant for a reaction with negative ∆H value decreases as the temperature increases.

Solution

The statement is incorrect. The reaction taking place in solution is:
Fe³⁺ (aq) + 3SCN^- (aq) ⇌ Fe(SCN)₃
Oxalic acid (H₂C₂O₄) reacts with Fe³⁺ (aq) present in solution to form the complex Fe(SCN)_3.As a result, the concentration of Fe³⁺ ions in the solution decreases and the intensity of red colour decreases.
Question 4
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A 50 ml solution of 0.1 M AgNO₃ is mixed with 50 ml of 0.01 M NaBrO₃ solution. K_sp of AgBrO₃ is 5.8 x 10^-5. Which of the following is correct?

A
Product of ionic concentrations is 2.5 x 10^-3.

B
AgBrO₃is not precipitated as the product of ionic concentrations is less than K_sp.

C
AgBrO₃is precipitated as the product of ionic concentrations is more than K_sp.

D
AgBrO₃is not precipitated as the product of ionic concentrations is more than K_sp.

Solution

Precipitation takes place when ionic product is more than solubility product.
Initial concentration of Ag⁺ ions = 0.1 M
Initial concentration of BrO₃^- ions = 0.01 M
Final volume of solution = 50 + 50 = 100 ml
Final [Ag⁺] = 0.1 × 50/100 = 0.05
Final [BrO₃^-] = 0.01 × 50/100 = 0.005
Product of ionic concentrations of AgBrO₃ = [Ag⁺] [BrO₃^-] = 0.05 × 0.005 = 2.5 × 10^-4, which is greater than the solubility product.
Hence, precipitate of AgBrO₃ will be formed.
Question 5
1 / -0

At 700 K, the equilibrium constant K_p for the reaction 2SO₃ (g) ⇌ 2SO₂(g) + O₂ is 1.8 x 10^–3 kPa. What is the numerical value in moles per liter of K_c for the reaction at the same temperature?

A
3.09 x 10^-7

B
4.09 x 10^-7

C
5.25 x 10^-7

D
4.75 x 10^-7

Solution

K_p = Kc (RT)^∆n
K_c = Kp/(RT)^∆n
T = 700 K
R = 8.314 J mol^-1_K^-1
∆n = (2 + 1) – 2 = 1
K_p = 1.8 X 10^-3kPa = 1.8 Pa
Therefore,
K_c = 1.8 Pa / (8.314 J mol^-1 K^-1) (700)¹
= 3.09 X 10^-7 mol m^-3
Hence, the numerical value in moles per liter of K_c is equal to 3.09 X 10^-7 mol m^-3.

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Chemical Equilibrium Test - 4

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Chemical Equilibrium Test - 4

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Question 1

Equilibrium is possible only in a closed system at a given temperature.

All measurable properties of the system remain constant.

All the physical processes stop at equilibrium.

The opposing processes occur at the same rate and there is a dynamic but stable condition.

Solution

Question 2

Freezing of ice in a open vessel, where the temperature of ice is constant.

A few drops of water are present along with air in a balloon, where the temperature of the balloon is constant.

Water is boiling in an open vessel over stove, where the temperature of water is constant.

All of these

Solution

Question 3

In an equilibrium mixture of ice and water kept in a perfectly insulated flask, the masses of ice and water do not change with time.

The intensity of red colour increases when oxalic acid is added to a solution containing iron (III) nitrate and potassium thiocyanate.

On addition of catalyst, the equilibrium constant value is not affected.

Equilibrium constant for a reaction with negative ∆H value decreases as the temperature increases.

Solution

Question 4

Product of ionic concentrations is 2.5 x 10-3.

AgBrO3 is not precipitated as the product of ionic concentrations is less than Ksp.

AgBrO3 is precipitated as the product of ionic concentrations is more than Ksp.

AgBrO3 is not precipitated as the product of ionic concentrations is more than Ksp.

Solution

Question 5

3.09 x 10-7

4.09 x 10-7

5.25 x 10-7

4.75 x 10-7

Solution

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Product of ionic concentrations is 2.5 x 10^-3.

AgBrO₃is not precipitated as the product of ionic concentrations is less than K_sp.

AgBrO₃is precipitated as the product of ionic concentrations is more than K_sp.

AgBrO₃is not precipitated as the product of ionic concentrations is more than K_sp.

3.09 x 10^-7

4.09 x 10^-7

5.25 x 10^-7

4.75 x 10^-7