$A$ sample of $HI_{(g)}$ is placed in a flask at a pressure of $0.2 \ atm$. At equilibrium,the partial pressure of $HI_{(g)}$ is $0.04 \ atm$. What is $K_{p}$ for the given equilibrium?
$2 HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$
$2 HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$
(4.0) The initial pressure of $HI$ is $0.2 \ atm$. At equilibrium,it has a partial pressure of $0.04 \ atm$. The decrease in the pressure of $HI$ is $0.2 - 0.04 = 0.16 \ atm$.
The reaction is: $2HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$
Initial pressure: $0.2 \ atm, 0, 0$
At equilibrium: $0.04 \ atm, \frac{0.16}{2} \ atm, \frac{0.16}{2} \ atm$
At equilibrium: $0.04 \ atm, 0.08 \ atm, 0.08 \ atm$
$K_{p} = \frac{p_{H_{2}} \times p_{I_{2}}}{p_{HI}^2}$
$K_{p} = \frac{0.08 \times 0.08}{(0.04)^{2}} = \frac{0.0064}{0.0016} = 4.0$
Hence,the value of $K_{p}$ is $4.0$.
The reaction is: $2HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$
Initial pressure: $0.2 \ atm, 0, 0$
At equilibrium: $0.04 \ atm, \frac{0.16}{2} \ atm, \frac{0.16}{2} \ atm$
At equilibrium: $0.04 \ atm, 0.08 \ atm, 0.08 \ atm$
$K_{p} = \frac{p_{H_{2}} \times p_{I_{2}}}{p_{HI}^2}$
$K_{p} = \frac{0.08 \times 0.08}{(0.04)^{2}} = \frac{0.0064}{0.0016} = 4.0$
Hence,the value of $K_{p}$ is $4.0$.
Explore More
Similar Questions
At $600\ ^{\circ}C$,$NH_4COONH_2\ (s) \rightleftharpoons 2NH_3\ (g) + CO_2\ (g)$ has an equilibrium constant $K_p = 3.2 \times 10^2\ bar^3$. Calculate $K_c$. $\left( R = 0.082\ L\ atm\ K^{-1}\ mol^{-1} \right)$
Medium
View SolutionAt $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.
In which of the following equilibria,$K_p$ and $K_c$ are $NOT$ equal?
MediumNEET 2024
View Solution$18.4 \ g$ of $N_2O_4$ was placed in a $1 \ L$ vessel at $400 \ K$ and allowed to attain the following equilibrium: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. If the total pressure at equilibrium was $10.64 \ bar$,the approximate $K_p$ is (Given: $R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$,assume $N_2O_4$ and $NO_2$ behave as ideal gases).
For the reaction $MgCO_{3(s)} \rightleftharpoons MgO_{(s)} + CO_{2(g)}$,the value of $K_p$ is:
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo