Question

[Review Topics References Use the References to access important value if needed for this question. Consider the following system at equilibrium at 698 K: 2 HI(g) + 2.49 kcal = H, (g) +13 (8) Indicate whether each individual change would favor the production of H, (g). Evaluate each change separately, assuming that all other conditions remain constant. Decreasing the temperature. Decreasing the pressure. Decreasing the volume. Removing HI Removing I, Suomet Answer Retry Entire Group 7 more group attempts remaining

please help it is suppose to be yes and no answers and I'm confused

Answer 1

1)

Decreasing Temperature will shift the reaction in a direction which release heat as per Le chatelier Principle

Forward reaction is endothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

Production of H2 is not favoured

Answer: no

2)

Decrease the pressure will shift the reaction in a direction which have greater gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is same on both side

So equilibrium will not be effected

So, No effect on equilibrium

Production of H2 is not favoured

Answer: no

3)

Decreasing volume will increase the pressure which in turn shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is same on both side

So equilibrium will not be effected

So, No effect on equilibrium

Production of H2 is not favoured

Answer: no

4)

Removing reactant will shift the reaction in the direction of reactant as per Le chatelier Principle

So, Equilibrium moves to reactant side

Production of H2 is not favoured

Answer: No

5)

Removing product will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

Production of H2 is favoured

Answer: yes