(B) Given reaction: $N_2 + 3H_2 \rightleftharpoons 2NH_3$Initial moles: $n(N_2) = 1, n(H_2) = 1, n(NH_3) = 1$Let $x$ be the moles of $N_2$ reacted at

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

(B) Given reaction: $N_2 + 3H_2 \rightleftharpoons 2NH_3$Initial moles: $n(N_2) = 1, n(H_2) = 1, n(NH_3) = 1$Let $x$ be the moles of $N_2$ reacted at equilibrium.Equilibrium moles of $N_2 = 1 - x = 0.7 \Rightarrow x = 0.3 \ mol$Equilibrium moles of $H_2 = 1 - 3x = 1 - 3(0.3) = 0.1 \ mol$Equilibrium moles of $NH_3 = 1 + 2x = 1 + 2(0.3) = 1.6 \ mol$Since volume $V = 1 \ L$,concentrations are equal to the number of moles.$[N_2] = 0.7 \ M, [H_2] = 0.1 \ M, [NH_3] = 1.6 \ M$Equilibrium constant $K_c = \frac{[NH_3]^2}{[N_2][H_2]^3}$$K_c = \frac{(1.6)^2}{(0.7)(0.1)^3} = \frac{2.56}{0.7 \times 0.001} = \frac{2.56}{0.0007} = 3657.14$

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

Difficult

Consider the following reaction in a $1 \ L$ closed vessel: $N_2 + 3H_2 \rightleftharpoons 2NH_3$. If all the species $N_2, H_2$ and $NH_3$ are $1 \ mol$ each at the beginning of the reaction and equilibrium is attained when unreacted $N_2$ is $0.7 \ mol$,what is the value of the equilibrium constant?

TS EAMCET 2018 All TS EAMCET

A
$3600$
B
$3657.14$
C
$2657.14$
D
$1828.57$

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

Previous Year

TS EAMCET 2018 Paper All TS EAMCET years →

When $3 \ mol$ of $A$ and $1 \ mol$ of $B$ are mixed in a $1 \ L$ vessel,the following reaction takes place: $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$. If $1.5 \ mol$ of $C$ are formed at equilibrium,the equilibrium constant $(K_c)$ for the reaction is:

Medium

View Solution

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:
$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$
$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
What is the relationship between $K_1$ and $K_2$?

DifficultAIPMT 2005

View Solution

$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$
In an equilibrium mixture,the partial pressures are
$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and
$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

MediumJEE MAIN 2021

View Solution

One mole $H_2O_{(g)}$ and one mole $CO_{(g)}$ are taken in a $1 \ L$ flask and heated to $725 \ K$. At equilibrium,$40 \%$ of water reacted with $CO_{(g)}$ as follows:
$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$
Its $K_c$ value is:

MediumAP EAMCET 2023

View Solution

At $1050 \ K$,for the chemical reaction $FeO_{(s)} + CO_{(g)} \rightleftharpoons Fe_{(s)} + CO_{2_{(g)}}$; $K_p = 0.25$. What are the equilibrium partial pressures of $CO_{(g)}$ and $CO_{2_{(g)}}$ at $1050 \ K$,if the initial partial pressures are: $P_{CO_{(g)}} = 1.6 \ atm$ and $P_{CO_{2_{(g)}}} = 0.8 \ atm$?

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

Similar Questions

When $3 \ mol$ of $A$ and $1 \ mol$ of $B$ are mixed in a $1 \ L$ vessel,the following reaction takes place: $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$. If $1.5 \ mol$ of $C$ are formed at equilibrium,the equilibrium constant $(K_c)$ for the reaction is:

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$What is the relationship between $K_1$ and $K_2$?

$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$In an equilibrium mixture,the partial pressures are$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

One mole $H_2O_{(g)}$ and one mole $CO_{(g)}$ are taken in a $1 \ L$ flask and heated to $725 \ K$. At equilibrium,$40 \%$ of water reacted with $CO_{(g)}$ as follows:$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$Its $K_c$ value is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:
$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$
$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
What is the relationship between $K_1$ and $K_2$?

$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}$
In an equilibrium mixture,the partial pressures are
$P_{SO_{3}} = 43 \ kPa$,$P_{O_{2}} = 530 \ Pa = 0.53 \ kPa$,and
$P_{SO_{2}} = 45 \ kPa$. The equilibrium constant $K_{p} = ...... \times 10^{-2} \ kPa^{-1}$. (Nearest integer)

One mole $H_2O_{(g)}$ and one mole $CO_{(g)}$ are taken in a $1 \ L$ flask and heated to $725 \ K$. At equilibrium,$40 \%$ of water reacted with $CO_{(g)}$ as follows:
$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)}$
Its $K_c$ value is: