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Equilibrium — Chemistry STD 11 Science — Question

Gujarat BoardEnglish MediumSTD 11 ScienceChemistryEquilibrium5 Marks
Question
Consider the following equilibrium at 2773K
$\text{H}_2(\text{g})+\text{Cl}_2(\text{g})\rightleftharpoons2\text{HCl}(\text{g})$
Initially $0.25M H_2$ and $0.25MCl_2$ are introduced into a reaction vessel and the system in allowed to attain equilibrium. At equilibrium the concentrations of $H_2(g)$ and $Cl_2(g)$ became $0.0314M$. Calculate $K_c$ and $K_p$.
✓

Answer

  1. $\begin{matrix}&\text{H}_2(\text{g})&+&\text{Cl}_2(\text{g})\rightleftharpoons&\text{2Hcl}(\text{g})\\\text{Initial Conc. }&0.25&&0.25\text{M}&0\\\text{Final Conc.at equilibrium}&0.0314\text{M}&&0.0314\text{M}&0\end{matrix}$
$2(0.25-0.0314)=0.2186\text{M}\times2$

$=0.219\text{M}\times2=0.438$

$\text{K}_{\text{c}}=\frac{[\text{HCl}]^2}{[\text{H}_2][\text{Cl}_2]}$

$=\frac{(0.438)^2}{0.0314\times0.314}=195$
  1. $\text{K}_{\text{p}}=\text{K}_{\text{c}}(\text{RT})^{\Delta\text{n}}$
$\Delta\text{n}=0$

$\text{K}_{\text{p}}=\text{K}_{\text{c}}=195$

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