What will be the difference in heat at constant pressure and constant volume for the combustion of carbon monoxide at $27 \, ^oC$ in $cal$?

For a phase change$H _2 O ( l ) \underset{1 bar , 0^{\circ} C }{\rightleftharpoons} H _2 O ( s )$

In an exothermic reaction,the reactants:

Expansion of a gas in vacuum is called free expansion. Calculate the work done and the change in internal energy when $1 \ L$ of ideal gas expands isothermally into vacuum until its total volume is $5 \ L$?

Calculate work done in isothermal reversible expansion of $1 \ mol$ of an ideal gas from an initial pressure of $10 \ bar$ to a final pressure of $1 \ bar$ at $300 \ K$ $\left(R = 8.314 \ J \ K^{-1} \ mol^{-1}\right)$. (in $kJ$)

$A$ system is changed from state $A$ to state $B$ by one path and from $B$ to $A$ by another path. If $E_1$ and $E_2$ are the corresponding changes in internal energy,then: