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? $(1 \ L \cdot atm = 101 \ J)$

Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero)

For an ideal gas,the heat of reaction at constant pressure and heat of reaction at constant volume are related by the equation:

For an isochoric process,the first law of thermodynamics can be expressed as:

In an adiabatic process,no transfer of heat takes place between the system and surroundings. Choose the correct option for the free expansion of an ideal gas under adiabatic conditions from the following: