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(A) According to the kinetic theory of gases,the temperature of an ideal gas is directly proportional to the average translational kinetic energy of i

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Average kinetic energy of gas molecules

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(A) According to the kinetic theory of gases,the temperature of an ideal gas is directly proportional to the average translational kinetic energy of its molecules.The relationship is given by the equation:$KE_{	ext{avg}} = \frac{3}{2} k_{B} T$Where:$KE_{	ext{avg}}$ is the average translational kinetic energy,$k_{B}$ is the Boltzmann constant,$T$ is the absolute temperature of the gas.Therefore,temperature is a measure of the average kinetic energy of the gas molecules.

The temperature of a gas is a measure of .........

Similar Questions

The temperature at which the kinetic energy of oxygen molecules becomes double its value at $27^{\circ}\,C$ is $............^{\circ}\,C$.

$A$ gas at a pressure ${P_0}$ is contained in a vessel. If the masses of all the molecules are halved and their speeds are doubled,the resulting pressure $P$ will be equal to:

The translational kinetic energy of the molecules of a gas at absolute temperature $T$ can be doubled by:

The average translational kinetic energy of the oxygen molecules at a temperature of $127^{\circ} C$ is (Boltzmann constant $= 1.38 \times 10^{-23} \,J \,K^{-1}$)

Assertion $(A)$: The temperature of a gas is a result of the kinetic energy of its molecules.
Reason $(R)$: Due to kinetic energy,the molecules collide with each other to produce thermal energy.

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