For the reaction $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)$ at constant temperature,the value of $\Delta H - \Delta U$ is:

When $1 \, \text{mole}$ of monoatomic ideal gas at $T \, \text{K}$ undergoes adiabatic change under a constant external pressure of $1 \, \text{atm}$ and changes volume from $1 \, \text{L}$ to $2 \, \text{L}$,the final temperature in Kelvin would be:

The relation $q = -w$ is $NOT$ true for which of the following processes?

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $2.5 \ atm$ from $2.5 \ L$ to $4.5 \ L$. The change in internal energy of the gas in joules is: (in $J$)

For a gaseous reaction,$A_{(g)} + 3B_{(g)} \to 3C_{(g)} + 3D_{(g)}$. The value of $\Delta E$ is $17 \ kcal$ at $27 \ ^oC$. The value of $\Delta H$ in $kcal$ will be:

$A$ system receives $100 \ cal$ of heat,and at the same time,$50 \ cal$ of work is done by the system. Calculate the change in internal energy. (in $cal$)