Question

For the reaction H₂(g) + I₂(g) ↔ 2 HI(g), K = 794 at 298 K and 54 at 700 K. Is the formation of product HI favored more at the higher or the lower temperature?

Answer 1

The formation of product HI is favored more at the lower temperature of 298 K since the equilibrium constant is larger (K = 794) compared to the higher temperature of 700 K where K is 54.

Step-by-step explanation:

For the reaction H₂(g) + I₂(g) ↔ 2 HI(g), we are given that the equilibrium constant (K) is 794 at 298 K and 54 at 700 K. The equilibrium constant is a measure of the extent to which a reaction proceeds to products at a given temperature. A larger value of K indicates that the formation of products is more favored at equilibrium. Thus, at the lower temperature of 298 K (with the larger K value of 794), the formation of the product hydrogen iodide (HI) is more favored.

The equilibrium shifts to favor the exothermic reaction or the formation of products when the temperature is decreased, thereby favoring the formation of HI at lower temperatures. Conversely, increasing the temperature favors the endothermic reaction or the reactants, so at a higher temperature of 700 K, the equilibrium shifts to reduce HI concentration.