Question

The value of $K_p$ for the reaction:
$2{H_2}_{\left(g\right)}=2{H_2}_{\left(g\right)}+{S_2}_{\left(g\right)}$ is $1.2\times {!0}^{-2}$ at ${1065}^{o}C$. The value for $K_C$ is:

• A. $<1.2\times {10}^{-2}$
• B. $>1.2\times {10}^{-2}$
• C. $1.2\times {10}^{-2}$
• D. $0.12\times {10}^{-2}$

Answer 1

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

For the given reaction,

$2H_{2}S\left(g\right)\rightleftharpoons 2H_2\left(g\right)+S_2\left(g\right)$

$\Delta n=3-2=1$

$K_c=\frac{K_p}{{\left(RT\right)}^n}$

$=\frac{1.2\times {10}^{-2}}{{\left(RT\right)}^1}$

$\therefore$ $K_c<K_p$ or $K_c<1.2\times {10}^{-2}$

Hence, option A is correct