If the pressure of an ideal gas is doubled while keeping the volume constant, what happens to the rms speed of the gas molecules?

The translatory kinetic energy of a gas per $g$ is

Read the given statements and decide which is/are correct on the basis of kinetic theory of gases

(I) Energy of one molecule at absolute temperature is zero

(II) $r.m.s.$speeds of different gases are same at same temperature

(III) For one gram of all ideal gas kinetic energy is same at same temperature

(IV) For one mole of all ideal gases mean kinetic energy is same at same temperature

The average kinetic energy of a helium atom at ${30^ \circ }C$ is

$125\;ml$ of gas $A$ at 0.60 atmosphere and $150\;ml$ of gas $B$ at 0.80 atmospheric pressure at same temperature is filled in a vessel of $1\;litre$ volume. What will be the total pressure of mixture at the same temperature

At what temperature, the mean kinetic energy of ${O_2}$ will be the same for ${H_2}$ molecules at $- {73^ \circ }C$

Mean kinetic energy (or average energy) per $g$ molecule of a monoatomic gas is given by

Relationship between $P,V,$ and $E$ for a gas is

$125\;ml$ of gas $A$ at 0.60 atmosphere and $150\;ml$ of gas $B$ at 0.80 atmospheric pressure at same temperature is filled in a vessel of $1\;litre$ volume. What will be the total pressure of mixture at the same temperature

The temperature at which the average translational kinetic energy of a molecule is equal to the energy gained by an electron in accelerating from rest through a potential difference of $1\;volt$ is

A gas undergoes a process where its pressure increases linearly with volume, $P = aV + b$, where $a$ and $b$ are positive constants. If the initial volume is $V_0$ and the final volume is $2V_0$, what is the work done by the gas during this process?