Which of the following relations is correct for an ideal gas?
- A$P = \frac{2}{3} \frac{V}{N} \overline{E}$
- B$P = \frac{3}{2} \frac{V}{N} \overline{E}$
- C$P = \frac{2}{3} \frac{N}{V} \overline{E}$
- D$P = \frac{3}{2} \frac{N}{V} \overline{E}$
Explore More
Similar Questions
At what temperature $T$ will the kinetic energy of $0.3 \ mol$ of $He$ be equal to the kinetic energy of $0.4 \ mol$ of $Ar$ at $400 \ K$ (in $K$)?
Easy
View SolutionThe average kinetic energy of one molecule of an ideal gas at $27^{\circ} C$ and $1 \ atm$ pressure is
$A$ helium atom is two times heavier than a hydrogen molecule. At $298 \ K$,the average kinetic energy of helium is:
At the same temperature, the molecular speeds of two gases are $u_1$ and $u_2$, and their masses are $m_1$ and $m_2$, respectively. Which of the following expressions is correct?
Medium
View SolutionOne mole of oxygen at $273 \ K$ and one mole of sulphur dioxide at $546 \ K$ are taken in two separate containers,then:
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