(A) The reaction is $PCl_5 \rightleftharpoons PCl_3 + Cl_2$. Initial moles: $a, 0, 0$. At equilibrium: $a(1-\alpha), a\alpha, a\alpha$. Total moles at

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(A) The reaction is $PCl_5 \rightleftharpoons PCl_3 + Cl_2$. Initial moles: $a, 0, 0$. At equilibrium: $a(1-\alpha), a\alpha, a\alpha$. Total moles at equilibrium = $a(1-\alpha) + a\alpha + a\alpha = a(1+\alpha)$. Given $\alpha = 0.25$. Total moles = $a(1+0.25) = 1.25a$. Mole fraction of $Cl_2$ $(X_{Cl_2})$ = $\frac{a\alpha}{a(1+\alpha)} = \frac{0.25}{1.25} = \frac{1}{5} = 0.2$. Partial pressure of $Cl_2$ = $X_{Cl_2} \times P_{total} = 0.2 \times 2.0 \ atm = 0.4 \ atm$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Degree of dissociation and Vapour density

Easy

For the thermal dissociation of $PCl_5$ as $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,if '$a$' moles of $PCl_5$ are taken and at equilibrium,the degree of dissociation of $PCl_5$ is $0.25$ and the total pressure is $2.0 \ atm$,then the partial pressure of $Cl_2$ at equilibrium will be: (in $atm$)

A
$0.4$
B
$1.0$
C
$0.5$
D
$0.25$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

6-1.Equilibrium (Chemical Equilibrium)

Subtopic

Degree of dissociation and Vapour density

For the equilibrium reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $K_p$ is $2$. Calculate the percentage dissociation of $N_2O_{4(g)}$ at a total pressure of $0.5 \ atm$. (in $\%$)

Medium

View Solution

Calculate the degree of dissociation $\alpha$ for $0.1 \, N \, CH_3COOH$ (dissociation constant $K_a = 1 \times 10^{-5}$).

Medium

View Solution

At $T \, ^\circ C$,the vapour density of $PCl_5$ is $104.25$. The degree of dissociation of $PCl_5$ is ....$\%$

Medium

View Solution

$A$ $1 \ L$ vessel contains $2 \ moles$ of $PCl_5$ initially. If $K_c$ is found to be $1$,the degree of dissociation of $PCl_5$ for the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ is:

Medium

View Solution

Which of the following will have the highest degree of dissociation for $4-$nitrophenol in an aqueous solution (in $M$)?

Medium

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

For the thermal dissociation of $PCl_5$ as $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,if '$a$' moles of $PCl_5$ are taken and at equilibrium,the degree of dissociation of $PCl_5$ is $0.25$ and the total pressure is $2.0 \ atm$,then the partial pressure of $Cl_2$ at equilibrium will be: (in $atm$)

Similar Questions

For the equilibrium reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $K_p$ is $2$. Calculate the percentage dissociation of $N_2O_{4(g)}$ at a total pressure of $0.5 \ atm$. (in $\%$)

Calculate the degree of dissociation $\alpha$ for $0.1 \, N \, CH_3COOH$ (dissociation constant $K_a = 1 \times 10^{-5}$).

At $T \, ^\circ C$,the vapour density of $PCl_5$ is $104.25$. The degree of dissociation of $PCl_5$ is ....$\%$

$A$ $1 \ L$ vessel contains $2 \ moles$ of $PCl_5$ initially. If $K_c$ is found to be $1$,the degree of dissociation of $PCl_5$ for the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ is:

Which of the following will have the highest degree of dissociation for $4-$nitrophenol in an aqueous solution (in $M$)?

Vedclass Test Series

Exam Paper Generator

Online Exam Module