Question

$\log \frac{K_P}{K_C}+\log RT=0$ is a relationship for the reaction:

• A. $PC{l}_5\left(g\right)\to PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
• B. $2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right)$
• C. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$
• D. $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$

Answer 1

The correct option is B $2S{O}_2\left(g\right)+O_2\left(g\right)\to 2S{O}_3\left(g\right)$

Using $K_p=K_C(RT{)}^{\Delta n_g}$
Taking log on both side
$log{K}_p=log{K}_c+\Delta n_g\log RT$
$\log \frac{K_P}{K_C}=\Delta n_g\log RT$
So, $\Delta n_g=-1$
$\Delta n_g=\text{Number of mole of gaseous product - Number of mole of gaseous reactant}$
So for reaction,
$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
$\Delta n_g=2-3=-1$
Hence option (b) is correct.