Question

The value of $K_p$ for the following reaction $2H_{2}S\left(g\right)\rightleftharpoons 2H_2\left(g\right)+S_2\left(g\right)is1.2\times {10}^{-2}at{106.5}^{o}C.$ The value of $K_C$ for this reaction is

• A. $1.2\times {10}^{-2}$
• B. $<1.2\times {10}^{-2}$
• C. 83
• D. $>1.2\times {10}^{-2}$

Answer 1

The correct option is B $<1.2\times {10}^{-2}$

$K_p=K_c(RT{)}^{△n};△n=1$
So $K_c$ will be less than $K_p.$