Question

In a 13 L vessel initially following reaction occur : $C\left(s\right)+S_2\left(g\right)\rightleftharpoons C{S}_2\left(g\right)$.

At equlibrium $12g=C,$ $64g=S_2$ and $76g=C{S}_2$ is present at ${1027}^{o}C$ temperature then total pressure is:

• A. $200R$
• B. $158R$
• C. $100R$
• D. $79R$

Answer 1

The correct option is A $200R$

Solution:- (A) $200R$

$C_{\left(s\right)}+{S_2}_{\left(g\right)}\rightleftharpoons {C{S}_2}_{\left(g\right)}$

Total no. of gaseous moles $=n_{S_2}+n_{C{S}_2}=2\text{moles}$

Volume $\left(V\right)=13L$

$T=1027℃=(1027+273)K=1300K$

Now, from ideal gas equation,

$PV=nRT$

$\Rightarrow P=\frac{nRT}{V}$

$\Rightarrow P=\frac{2\times R\times 1300}{13}=200R$

Hence the total pressure is $200R$.