$A$ gas at $10^{\circ}C$ occupies a volume of $283 \text{ mL}$. If it is heated to $20^{\circ}C$ at constant pressure, what is the new volume of the gas (in $\text{ mL}$)?

An ideal gas weighing $9.0 \ g$ occupies a volume of $8.2 \ L$ at $300 \ K$ and $1 \ atm$ pressure. The molar mass of the gas is .....

$4 \ g$ of an ideal gas $A$ (molar mass $= M_A$) present in a vessel of a volume $V \ L$ exerted a pressure of $5 \ atm$ at $300 \ K$. When $16 \ g$ of another ideal gas $B$ (molar mass $= M_B$) was introduced into this vessel at the same temperature, the pressure increased to $10 \ atm$. What is the correct relationship between $M_A$ and $M_B$?

For an ideal gas,the value of ${\left( {\frac{{dU}}{{dV}}} \right)_T}$ is ...... .

If the temperature of a gas is increased by $1\,^oC$ while keeping the pressure and the amount of gas constant,what is the change in the original volume of the gas?

In the equation $PV = nRT$,which of the following is not equal to the numerical value of $R$?