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Derivation of Kp and Kc

The equilibri...

Question

The equilibrium constant $K$ for the reaction : $2 H I (g) ⇌ H_{2} (g) + I_{2} (g)$ at room temperature is $2.85$ and that at $698 K$ is $1.4 \times {! 0}^{- 2}$ . This implies that the forward reaction is:

exothermic

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endothermic

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slow

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unpredictable

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Solution

The correct option is B exothermic
$2 H I_{(g)} ⇌ H_{2 ((g)} + I_{2 (g)}$
Room temperature $⟶ 285$
$698 K ⟶ 1.4 \times 10^{- 2}$
We can see that as the temperature increases, the value of $K_{p}$ falls.
Hence, the powered reaction is exothermic.

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