(C) Given reaction: $NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$ with $K_{c1} = 4$.For the target reaction: $N_{2(g)} +

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

$\left( \frac{1}{4 \times 800R} \right)^2$

(C) Given reaction: $NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$ with $K_{c1} = 4$.For the target reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,we reverse the first reaction and multiply by $2$.Thus,$K_{c2} = (1/K_{c1})^2 = (1/4)^2 = 1/16$.The relationship between $K_P$ and $K_c$ is $K_P = K_c(RT)^{\Delta n}$.For the target reaction,$\Delta n = 2 - (1 + 3) = -2$.Temperature $T = 527 + 273 = 800 \ K$.$K_P = (1/16) \times (R \times 800)^{-2} = (1/4)^2 \times (800R)^{-2} = \left( \frac{1}{4 \times 800R} \right)^2$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Medium

At $527 \ ^oC$,the reaction given below has $K_c = 4$.
$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$
What is the $K_P$ for the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

A
$16 \times (800 \ R)^2$
B
$\left( \frac{800R}{4} \right)^{-2}$
C
$\left( \frac{1}{4 \times 800R} \right)^2$
D
None of these

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

6-1.Equilibrium (Chemical Equilibrium)

Subtopic

Kp and Kc Relationship

When $4.5 \, \text{mol}$ each of hydrogen and iodine are heated in a $10 \, \text{L}$ closed vessel,$3 \, \text{mol}$ of $HI$ are formed at equilibrium. The equilibrium constant $K_c$ for the reaction ${H_2} + {I_2} \rightleftharpoons 2HI$ is .........

Medium

View Solution

For the reaction $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)},$ if $K_P = K_C (RT)^x$ where the symbols have usual meaning,then the value of $x$ is (assuming ideality):

MediumJEE MAIN 2014

View Solution

For the reaction ${H_2}_{(g)} + {I_2}_{(g)} \rightleftharpoons 2HI_{(g)}$ at $721 \ K$,the value of the equilibrium constant $({K_c})$ is $50$. When the equilibrium concentration of both is $0.5 \ M$,the value of ${K_p}$ under the same conditions will be:

MediumAIPMT 1990

View Solution

At $1990 \ K$ and $1 \ atm$ pressure,there are equal number of $Cl_2$ molecules and $Cl$ atoms in the reaction mixture. The value $K_P$ for the reaction $Cl_{2(g)} \rightleftharpoons 2Cl_{(g)}$ under the above conditions is $x \times 10^{-1}$. The value of $x$ is ..........
(Rounded off to the nearest integer)

EasyJEE MAIN 2021

View Solution

The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

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

At $527 \ ^oC$,the reaction given below has $K_c = 4$.$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$What is the $K_P$ for the following reaction?$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

Similar Questions

When $4.5 \, \text{mol}$ each of hydrogen and iodine are heated in a $10 \, \text{L}$ closed vessel,$3 \, \text{mol}$ of $HI$ are formed at equilibrium. The equilibrium constant $K_c$ for the reaction ${H_2} + {I_2} \rightleftharpoons 2HI$ is .........

For the reaction $SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightleftharpoons SO_{3(g)},$ if $K_P = K_C (RT)^x$ where the symbols have usual meaning,then the value of $x$ is (assuming ideality):

For the reaction ${H_2}_{(g)} + {I_2}_{(g)} \rightleftharpoons 2HI_{(g)}$ at $721 \ K$,the value of the equilibrium constant $({K_c})$ is $50$. When the equilibrium concentration of both is $0.5 \ M$,the value of ${K_p}$ under the same conditions will be:

The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

At $527 \ ^oC$,the reaction given below has $K_c = 4$.
$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$
What is the $K_P$ for the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$