(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G^o$ must be negative.The relationship is given by $\Delta G^o = \Delta H^o

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

(C) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G^o$ must be negative.The relationship is given by $\Delta G^o = \Delta H^o - T \Delta S^o$.At equilibrium,$\Delta G^o = 0$,so $T = \frac{\Delta H^o}{\Delta S^o}$.Given $\Delta H^o = 491.1 \ kJ \ mol^{-1} = 491100 \ J \ mol^{-1}$ and $\Delta S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$.$T = \frac{491100 \ J \ mol^{-1}}{198.0 \ J \ K^{-1} \ mol^{-1}} = 2480.3 \ K$.Therefore,the reaction becomes spontaneous at temperatures above $2480.3 \ K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Difficult

The reaction $MgO_{(s)} + C_{(s)} \to Mg_{(s)} + CO_{(g)}$,for which $\Delta_r H^o = +491.1 \ kJ \ mol^{-1}$ and $\Delta_r S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$,is not feasible at $298 \ K$. The temperature above which the reaction will be feasible is ..... $K$.

JEE MAIN 2019 All JEE MAIN

A
$2040.5$
B
$1890$
C
$2480.3$
D
$2380.5$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

Thermodynamics

Subtopic

Free energy and Work

Previous Year

JEE MAIN 2019 Paper All JEE MAIN years →

For a certain reaction, $\Delta H^0 = -345 \text{ kJ}$ and $\Delta S^0 = -123 \text{ JK}^{-1}$. At what temperature will the change over from spontaneous to non-spontaneous occur (in $\text{ K}$)?

DifficultMHT CET 2026

View Solution

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

Easy

View Solution

For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

Medium

View Solution

The enthalpy and entropy change for the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$ are $30 \ kJ \ mol^{-1}$ and $105 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature at which the reaction will be in equilibrium is ............... $K$.

MediumAIPMT 2006

View Solution

For a process occurring at constant temperature and pressure,which of the following is true at equilibrium?

Easy

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

The reaction $MgO_{(s)} + C_{(s)} \to Mg_{(s)} + CO_{(g)}$,for which $\Delta_r H^o = +491.1 \ kJ \ mol^{-1}$ and $\Delta_r S^o = 198.0 \ J \ K^{-1} \ mol^{-1}$,is not feasible at $298 \ K$. The temperature above which the reaction will be feasible is ..... $K$.

Similar Questions

For a certain reaction, $\Delta H^0 = -345 \text{ kJ}$ and $\Delta S^0 = -123 \text{ JK}^{-1}$. At what temperature will the change over from spontaneous to non-spontaneous occur (in $\text{ K}$)?

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:

The enthalpy and entropy change for the reaction $Br_{2(l)} + Cl_{2(g)} \rightarrow 2BrCl_{(g)}$ are $30 \ kJ \ mol^{-1}$ and $105 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature at which the reaction will be in equilibrium is ............... $K$.

For a process occurring at constant temperature and pressure,which of the following is true at equilibrium?

Vedclass Test Series

Exam Paper Generator

Online Exam Module