If Kc for the formation of HI from H2 and I2 each is 64, then calculat

1.	If Kc for the formation of HI from H2 and I2 each is 64, then calculate Kc for the decomposition of 1 mole of HI.
Answer» H₂(g) + I₂(g) \(\rightleftharpoons\) 2HI(g) using law of mass action- K_c = \(\frac{[HI]^2}{[H_2][I_2]}\) = 64-----(i) for decomposition of one mole of HI--- HI(g) \(\rightleftharpoons\) 1/2 H₂(g) + 1/2 I₂(g) K'_c = \(\frac{[H_2]^{1/2}[I_2]^{1/2}}{[HI]}\)----(ii) using equation (i) & (ii)--- K'_c = \(\frac{1}{\sqrt{K_c}}\) K'_c= \(\frac1{\sqrt{64}}\) K'_c= 1/8 K'_c = 0.125 Hence, K'_c for the decomposition of 1 mole of HI will be 0.125.

If Kc for the formation of HI from H2 and I2 each is 64, then calculate Kc for the decomposition of 1 mole of HI.

Answer»

H₂(g) + I₂(g) \(\rightleftharpoons\) 2HI(g)

using law of mass action-

K_c = \(\frac{[HI]^2}{[H_2][I_2]}\) = 64-----(i)

for decomposition of one mole of HI---

HI(g) \(\rightleftharpoons\) 1/2 H₂(g) + 1/2 I₂(g)

K'_c = \(\frac{[H_2]^{1/2}[I_2]^{1/2}}{[HI]}\)----(ii)

using equation (i) & (ii)---

K'_c = \(\frac{1}{\sqrt{K_c}}\)

K'_c= \(\frac1{\sqrt{64}}\)

K'_c= 1/8

K'_c = 0.125

Hence, K'_c for the decomposition of 1 mole of HI will be 0.125.

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If Kc for the formation of HI from H2 and I2 each is 64, then calculate Kc for the decomposition of 1 mole of HI.

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