Question

$0.5$ ml of $H_2$ and $0.5$ mole of $I_2$ react in $10$ litre flask at ${448}^o$C. The equilibrium constant $K_c$ is $50$ for $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$

What is the value of $K_p$?

• A. 50
• B. 20
• C. 10
• D. 40

Answer 1

The correct option is A 50

The given reaction is :-

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

we have, $K_P=K_C{\left(RT\right)}^{△n}$

$△n=$ No. of moles of gaseous (product - reactant)

$=2-1-1=0$

$\Rightarrow K_P=K_C{\left(RT\right)}^0\Rightarrow K_P=K_C=50$.