One mole of an ideal gas for which $C_v = (3/2)R$ is heated at a constant pressure of $1 \ atm$ from $25 \ ^oC$ to $100 \ ^oC$. The value of $\Delta H$ is $...... \ cal$.

Two moles of an ideal monoatomic gas are allowed to expand adiabatically and reversibly from $300 \ K$ to $200 \ K$. The work done in the process will be $..... \ kJ$.

The difference between the reaction enthalpy change $(\Delta _r H)$ and reaction internal energy change $(\Delta _r U)$ for the reaction $2C_6H_{6(l)} + 15O_{2(g)} \longrightarrow 12CO_{2(g)} + 6H_2O_{(l)}$ at $300 \ K$ is $....$ $J \ mol^{-1}$ $(R = 8.314 \ J \ mol^{-1} \ K^{-1})$

In an adiabatic process,the work involved during expansion or compression of an ideal gas is given by

Two statements are given below.
Statement $I$: The reaction $Cr_2O_3 + 2 Al \rightarrow Al_2O_3 + 2 Cr$ $(\Delta G^{\ominus} = -421 \ kJ)$ is thermodynamically feasible.
Statement $II$: The above reaction occurs at room temperature.
The correct answer is

$10 \, mol$ of an ideal gas expands isothermally and reversibly from a pressure of $10 \, atm$ to $1 \, atm$ at $300 \, K$. What is the largest mass (in $kg$) which can be lifted through a height of $100 \, m$ by the energy obtained in this process (in $, kg$)?