For a certain chemical reaction, ΔH∘=-156kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.

a. Increase the temperature.

b. Decrease the temperature.

Question

Kenley

Chemistry

26 December, 01:53

For a certain chemical reaction, ΔH∘=-156kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.

a. Increase the temperature.

b. Decrease the temperature.

+5

Answers (1)

Know the Answer?

Kiera Chandler · Answer 1

As per Le Chatelier's principle, any disturbance caused in an equilibrium reaction will tend to shift the equilibrium in a direction away from the disturbance.

Since, the given reaction is exothermic in nature so, when we increase the temperature then reaction will shift in the direction opposing the increase in temperature. Hence, the equilibrium will shift on left side when we increase the temperature.

On the other hand, when we decrease the temperature then the equilibrium will shift on the right side.

For a certain chemical reaction, ΔH∘=-156kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.a. Increase the temperature.b. Decrease the temperature.

For a certain chemical reaction, ΔH∘=-156kJ. Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.

a. Increase the temperature.

b. Decrease the temperature.