Question

1 mole of gas $AB$ dissociates to an extent of $10\%$ at ${127}^{0}C$ according to $AB\rightleftharpoons A+B$ occupies a volume of $4\times {10}^{4}ml$. Find the total pressure at this temp, assuming ideal gas behaviour.

Answer 1

The given reaction is :-

$AB\rightleftharpoons A+BT={127}^{0}C=127+273$

Initial moles : $1$ $0$ $0$ $=400K$

At eqm : $(1-0.1)$ $0.1$ $0.1$

$=0.9$

Total moles at equation $=0.9+0.1+0.1=1.1$

Now, By ideal gas equation, $PV=nRT$

$\Rightarrow P=\frac{nRT}{V}=\frac{1.1\times 0.0821\times 400}{40}=0.9031atm$