Question

two balloons hold two different gases. the gases are held at the same pressure, volume, and temperature. which quantity can differ between the two gases? (1 point) the mass of each gas the gas constant of each gas the molar volume of each gas the number of moles of each gas

Explanation:

Step1: Recall ideal gas law

The ideal - gas law is $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the gas constant, and $T$ is temperature. Given that $P$, $V$, and $T$ are the same for the two gases, from $PV=nRT$, we can see that $n$ (number of moles) must be the same for both gases since $R$ is a universal constant.

Step2: Consider molar volume

Molar volume $V_m=\frac{V}{n}$. Since $V$ and $n$ are the same for the two gases, the molar volume is the same.

Step3: Analyze gas constant

The gas constant $R$ is a universal constant and does not depend on the type of gas.

Step4: Analyze mass

The mass $m$ of a gas is related to the number of moles $n$ by $m = nM$, where $M$ is the molar mass. Since different gases have different molar masses $M$ and although $n$ is the same (from the ideal - gas law), the mass $m$ of each gas can be different.

Answer:

the mass of each gas