Question

1 mole of $H_2$, 2 moles of $I_2$ and 3 moles of HI were taken in 1 litre flask. The equilibrium constant of the reaction:

$H_{2\left(g\right)}+I_{2\left(g\right)}\rightleftharpoons 2H{I}_{\left(g\right)}$

is 50 at ${330}^{o}C$. The concentration of HI at equilibrium is:

• A. 0.3
• B. 1.6
• C. 4.4
• D. 2.7

Answer 1

The correct option is C 4.4

$\begin{array}{cc}2t& =\frac{(3{)}^2}{\left(2\right)}\\ & =4.5\end{array}$

$Keq=\frac{(3+2x{)}^2}{(1-2x)(2-x)}=\frac{[HI{]}^2}{\left[H_2\right]C{I}_2]}$

$\begin{array}{c}50=\frac{(2x+3{)}^2}{(1-x)(2-x)}\\ x=0.7\end{array}$

$\begin{array}{cc}\text{at equilibrium concentration of}& HI=3+2x\\ & =3+2\times 0.7\\ & =\underset{–}{4.4}\end{array}$