Chemical Equilibrium Test

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Chemical Equilibrium Test - 1

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Weekly Quiz Competition

Question 1
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When a reversible reaction is at equilibrium, one of its products' concentration is decreased. The equilibrium state

A
shifts in the direction of backward reaction

B
shifts in the direction of forward reaction

C
is not affected

D
moves in either direction

Solution

According to the Lechatelier's principle when a system at equilibrium is subjected to a change, the equilibrium shifts in the direction so as to undo the change.

Therefore, if the concentration of product is decreased,the forward reaction takes place so as to increase the concentration.
Question 2
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The Haber's process for the manufacture of ammonia is usually carried out at 450–500°C. If the temperature of 250°C was used instead of 450–500°C, then

A
no NH₃ would be formed at all

B
the percentage of NH₃ in the equilibrium mixture would be too low

C
a catalyst would not be used at 250°C

D
the rate of formation of NH₃ would be too slow

Solution

The optimum condition for the formation of NH3 by Haber's process requires that the temperature of the combination of N₂ and H₂ should be 450–500°C. If the temperature is 250°C, then the rate of formation of NH₃ would be too slow. If the temperature is above 500°C, then the equilibrium will shift towards the left because the reaction is exothermic.
Question 3
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Assertion: An increase in the volume of a system that results in a decrease in the total pressure will cause a shift to the side of the equilibrium with greater number of moles of the gas.

Reason: This counters the decrease in the total pressure.

A
Both A and R are true and R is the correct explanation of A.

B
Both A and R are true but R is not correct explanation of A.

C
A is true but R is false.

D
Both A and R are true.

Solution

According to Le Châtelier's principle, "The decrease in the total pressure will cause a shift to the side of the equilibrium with greater number of moles of the gas."
Question 4
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Assertion: A net reaction can occur only if a system is not at equilibrium.

Reason: All reactions occur to reach a state of equilibrium.

A
Both A and R are true and R is the correct explanation of A.

B
Both A and R are true but R is not correct explanation of A.

C
A is true but R is false.

D
Both A and R are false.

Solution

The law of chemical equilibrium define the direction in which a chemical reaction will proceed, as well as the quantities of reactants and products that will remain after the reaction comes to an end.
Question 5
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Which of the following reactions will proceed in forward direction if the volume of the container is increased?

A
H₂ + Cl₂ → 2HCl

B
CaCO₃→ CaO + CO₂

C
N₂ + 3H₂→ 2NH₃

D
N₂ + 2O₂→ N₂O₄

Solution

If the total volume of a container is increased, this means that the total pressure is decreased. The equilibrium will then shift to the side with more moles of gases. In option 2, since CaO and CaCO₃ are solids, we can assume that their concentration are constant. But CO₂ is a gas. Therefore, in this case, the reaction will proceed in forward direction.

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Chemical Equilibrium Test - 1

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Question 1

shifts in the direction of backward reaction

shifts in the direction of forward reaction

is not affected

moves in either direction

Solution

Question 2

no NH3 would be formed at all

the percentage of NH3 in the equilibrium mixture would be too low

a catalyst would not be used at 250°C

the rate of formation of NH3 would be too slow

Solution

Question 3

Both A and R are true and R is the correct explanation of A.

Both A and R are true but R is not correct explanation of A.

A is true but R is false.

Both A and R are true.

Solution

Question 4

Both A and R are true and R is the correct explanation of A.

Both A and R are true but R is not correct explanation of A.

A is true but R is false.

Both A and R are false.

Solution

Question 5

H2 + Cl2 → 2HCl

CaCO3 → CaO + CO2

N2 + 3H2 → 2NH3

N2 + 2O2 → N2O4

Solution

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no NH₃ would be formed at all

the percentage of NH₃ in the equilibrium mixture would be too low

the rate of formation of NH₃ would be too slow

H₂ + Cl₂ → 2HCl

CaCO₃→ CaO + CO₂

N₂ + 3H₂→ 2NH₃

N₂ + 2O₂→ N₂O₄