Question

$CC{l}_4\rightleftharpoons C+2C{l}_2$

The equilibrium constant $pK$ for the given reaction at $700$${}^{0}C$ is $0.76$ atm.

The initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of $1.20$atm at ${700}^{o}C$ is:

• A. $0.22$ atm
• B. $0.44$ atm
• C. $0.84$ atm
• D. $0.11$ atm

Answer 1

Answer: (C)

$0.84$ atm

Let the intial pressure of $CC{l}_4$ br '$p$'

$CC{l}_4\left(g\right)\to C\left(s\right)+C{l}_2\left(g\right)$

$p-x$ $x$ $x$

Since, total pressure at equilibrium is 1.2,

$p+x=1.20$ $p=1.2-x$

$K_p=\frac{x}{p-x}$

$0.76=\frac{x}{1.2-x-x}$

by sloving we get, $x=0.36$

$\therefore p=0.84atm$

Hence, the correct option is $\text{C}$