Question

Ina $13$ litres vessel initially following reaction occur $C\left(s\right)+S_2\left(g\right)\to C{S}_2$(g) by $12$ gm C, 64 gm $S_2$, $76$ gm $C{S}_2$ at $1027$ temperature, then total pressure is:

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

Answer 1

Answer: (A)

$200R$

$\underset{1mole}{C}\left(s\right)+\underset{1mole}{S_2}\left(g\right)⟶\underset{1mole}{C{S}_2}\left(g\right)$

Moles of $C=\frac{12}{12}=1$ ; moles of $C{S}_2=\frac{76}{76}=1$

Moles of $S_2=\frac{64}{64}=1$

Total number of gaseous moles= $2$ ($\because C\left(s\right)$ is not gas)

$Pv=nRT$

$\Rightarrow P=\frac{2\times R(1027+273)}{13}$

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

$P=200R$