Question

4.5 moles each of hydrogen and iodine are heated in a sealed 10 litre vessel. At equilibrium 3 moles of hydrogen iodide was found. The equilibrium constant for $H_{2\left(g\right)}+I_{2\left(g\right)}\rightleftharpoons 2{HI}_{\left(g\right)}$
1) 1 2) 10 3) 5 4) 0.33

Answer 1

The correct option is 1

We have,

4.5 moles each of hydrogen and iodine which is heated in a sealed 10litre vessel.

$H_2\left(g\right)+I_2\left(g\right)\leftrightharpoons 2HI\left(g\right)$

Since 1 mole of $H_2$ and one mole of $I_2$ combine to give 2 moles

of $HI$ then 3 moles of $HI$ would be formed by ICE table,

$K_C$ for the reaction at equlibrium is :

$=\frac{[HI{]}^2}{\left[H_2\right]\left[I_2\right]}$

$=\frac{[3{]}^2}{\left[3\right]\left[3\right]}$

$=1$