If $E$ is the kinetic energy per mole of an ideal gas and $T$ is the absolute temperature,then the universal gas constant is given as
- A$\frac{2 T}{3 E}$
- B$\frac{2 E}{3 T}$
- C$\frac{3 T}{2 E}$
- D$\frac{3 E}{2 T}$
Explore More
Similar Questions
The mean kinetic energy of the molecules of an ideal gas at $399^{\circ} C$ is $E$. The temperature at which the mean kinetic energy of its molecules will be $E/2$ is: (in $^{\circ} C$)
The average force applied on the walls of a closed container depends on temperature $(T)$ as ($T$ is the temperature of an ideal gas).
The energy of a gas per litre is $600 \text{ J}$. What will be its pressure?
DifficultMHT CET 2026
View SolutionThe average kinetic energy of hydrogen molecules at $300\, K$ is $E$. At the same temperature,the average kinetic energy of oxygen molecules will be
Medium
View SolutionThe total internal energy of $4$ moles of a diatomic gas at a temperature of $27^{\circ} C$ is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)
Vedclass 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