The difference between $C_p$ and $C_v$ can be derived using the empirical relation $H = U + PV$. Calculate the difference between $C_p$ and $C_v$ for $10$ moles of an ideal gas.

An ideal gas expands in volume from $1 \times 10^{-3} \ m^3$ to $1 \times 10^{-2} \ m^3$ at $300 \ K$ against a constant pressure of $1 \times 10^5 \ N \ m^{-2}$. The work done is

If a chemical reaction is accompanied by the evolution of heat,it is

$1 \ mol$ of an ideal gas expands isothermally and reversibly by decreasing pressure from $210 \ kPa$ to $105 \ kPa$ at $300 \ K$. What is the work done (in $J$)? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

The change in internal energy of a system depends upon

For which of the following reactions is $\Delta E = \Delta H$?