During the free expansion of an ideal gas in an isolated chamber,

The volume of a gas at $STP$ is $1.5 \ L$. When $300 \ J$ of heat is supplied to it at $1 \ atm$ pressure,its volume becomes $2 \ L$. What is the value of $\Delta U$ in $J$ for this process? $(1 \ L \cdot atm = 101 \ J)$

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $10 \ atm$ from an initial volume $4.2 \ L$ to $5.2 \ L$. The change in internal energy $\Delta E$ of the gas will be $:-$

If $Q$ is the heat liberated from the system and $W$ is the work done on the system,then the first law of thermodynamics can be written as:

$A$ gas expands from a volume of $4 \ L$ to $14 \ L$ against a constant external pressure of $1 \ atm$ in a cylinder with a frictionless piston. During this process,the gas absorbs $800 \ J$ of heat from the surroundings. Calculate the change in internal energy $\Delta E$ in $J$. (in $.7$)

The heat change for the following reaction at $298 \ K$ and at constant pressure is $+7.3 \ kcal$: $A_2B_{(s)} \to 2A_{(s)} + 1/2B_{2(g)}$,$\Delta H = +7.3 \ kcal$. The heat change at constant volume would be: