For a reaction,$\Delta H = 9.08 \, kJ/mol$ and $\Delta S = 35.7 \, J/K \cdot mol$. Which of the following statements is true?
- AIt is reversible and isothermal.
- BIt is reversible and exothermic.
- CIt is spontaneous and endothermic.
- DIt is spontaneous and exothermic.
Explore More
Similar Questions
Calculate the work done if $1 \ mole$ of an ideal gas is compressed isothermally and reversibly from $12 \ dm^3$ to $6 \ dm^3$ at $300 \ K$. $\left[R = 8.314 \ J \ K^{-1} \ mol^{-1}\right]$ (in $kJ$)
For a particular reversible reaction at temperature $T$,$\Delta H$ and $\Delta S$ were found to be both positive. If $T_e$ is the temperature at equilibrium,the reaction would be spontaneous when
MediumAIEEE 2010
View Solution$A$ reaction has both $\Delta H$ and $\Delta S$ negative. The rate of reaction
The dependence of Gibbs free energy on pressure for an isothermal process of an ideal gas is given by:
Medium
View SolutionThe values of $\Delta H$ and $\Delta S$ of a certain reaction are $-400 \text{ kJ mol}^{-1}$ and $-20 \text{ kJ mol}^{-1} \text{ K}^{-1}$ respectively. The temperature below which the reaction is spontaneous, is
MediumWBJEE 2014
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