When heat $Q$ is supplied to a diatomic gas of rigid molecules at constant volume,its temperature increases by $\Delta T$. The heat required to produce the same change in temperature at constant pressure is:

  • A
    $\frac{3}{2} Q$
  • B
    $\frac{5}{3} Q$
  • C
    $\frac{7}{5} Q$
  • D
    $\frac{2}{3} Q$

Explore More

Similar Questions

What is the value of $\frac{R}{C_P}$ for a diatomic gas?

For a gas,the difference between the two specific heats is $4150 \ J \ kg^{-1} \ K^{-1}$ and the ratio of the two specific heats is $1.4$. What is the specific heat of the gas at constant volume in units of $J \ kg^{-1} \ K^{-1}$?

For an ideal gas,the molar specific heat at constant pressure is $(7/2) R$. Find the ratio of the molar specific heat at constant pressure to the molar specific heat at constant volume.

One mole of an ideal gas $\left( \frac{C_P}{C_V} = \gamma \right)$ is heated according to the law $P = \alpha V$,where $P$ is the pressure of the gas,$V$ is the volume,and $\alpha$ is a constant. What is the molar heat capacity of the gas in this process?

The quantity of heat required to raise the temperature of one mole of a monoatomic gas by one degree Kelvin at constant volume is

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