Question

According to the reaction, $4$ mole of $A$ are mixed with $4$ mole of $B$ when $2$ mole of $C$ are formed at equilibrium.

$A+B\rightleftharpoons C+D$

Find the equilibrium constant.

• A. $\sqrt{2}$
• B. $2$
• C. $1$
• D. $4$

Answer 1

The correct option is C $1$

$A+B\rightleftharpoons C+D$

Initial moles $4$ $4$ $0$ $0$

At eq. $4-x$ $4-x$ $x$ $x$
$2$ moles of $C$ are formed at equilibrium.

$\therefore x=2$
Moles of $A$ remaining $=4-2=2$
Moles of $B$ remaining $=4-2=2$
The equilibrium constant, $K_c=\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}$

$K=\frac{2\times 2}{2\times 2}$

$K=1$