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(D) For an ideal gas,the equation of state is given by $PV = nRT$,where $n$ is the number of moles,$R$ is the universal gas constant,and $T$ is the ab

Vedclass · Accepted Answer

$P_{A} V_{A}=P_{B} V_{B}$

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(D) For an ideal gas,the equation of state is given by $PV = nRT$,where $n$ is the number of moles,$R$ is the universal gas constant,and $T$ is the absolute temperature.Since the gases are in thermal equilibrium,their temperatures are equal,so $T_{A} = T_{B} = T$.Both containers contain the same mass of the same gas,so the number of moles $n$ is the same for both,i.e.,$n_{A} = n_{B} = n$.Applying the ideal gas equation to both containers:For container $A$: $P_{A} V_{A} = nRT$For container $B$: $P_{B} V_{B} = nRT$Since the right-hand sides are equal $(nRT = nRT)$,we must have $P_{A} V_{A} = P_{B} V_{B}$.Therefore,the correct option is $D$.

$A$ gas container $A$ is in thermal equilibrium with another gas of the same mass in container $B$. If we denote the corresponding pressures and volumes by the suffixes $A$ and $B$,then which of the following statements is most likely to be true?

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