When a solvent is added to a solution,the heat of the solution $...$.

$A$ perfect gas $(0.1 \ mol)$ having $\overline{C}_{v}=1.50 \ R$ (independent of temperature) undergoes the transformation shown in the graph from point $1$ to point $4$. If each step is reversible,the total work done $(w)$ while going from point $1$ to point $4$ is $(-)$ . . . . . . $J$ (nearest integer). [Given: $R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$,$1 \ L \ atm = 101.3 \ J$]

The value of $\Delta H - \Delta E$ for the following reaction at $27 \ ^\circ C$ will be $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$

When $2$ moles of an ideal gas are expanded isothermally from a volume of $12.5 \ L$ to $15.0 \ L$ against a constant external pressure of $760 \ mm \ Hg$,calculate the amount of work done in joules. (in $J$)

Calculate the constant external pressure required to expand $2$ moles of an ideal gas from volume $15 \ dm^{3}$ to $20 \ dm^{3}$ if the amount of work done is $-600 \ J$. (in $bar$)

The change in internal energy of a system depends upon