A certain reaction is spontaneous at $85°\mathrm{C}$. The reaction is endothermic by $34 \mathrm{kJ}$. The minimum value of $\mathrm{\Delta S}$ for the reaction is:

For the reaction, $\frac{1}{2}{\mathrm{A}}_2+\frac{1}{2}{\mathrm{B}}_2\to \mathrm{AB}; \mathrm{\Delta H}=-50 \mathrm{kcal}$.

If the bond energies of ${\mathrm{A}}_2, {\mathrm{B}}_2$ and $\mathrm{AB}$ are $\mathrm{x}, \frac{\mathrm{x}}{2}$ and $\mathrm{x} \mathrm{kcal}$, respectively, the value of $\mathrm{x}$ is:

One mole of a non ideal gas undergoes a change of state $(2.0 \mathrm{atm}, 3.0 \mathrm{L}, 95 \mathrm{K})$$\to (4 \mathrm{atm}, 5\mathrm{L}, 245 \mathrm{K})$ with a change in the internal energy, $\mathrm{\Delta U}=30.0 \mathrm{L} \mathrm{atm}$. The change in enthalpy, $\mathrm{\Delta H}$ of the process in $\mathrm{L} \mathrm{atm}$ is:

[Hint: $\mathrm{\Delta H}=\mathrm{\Delta U}+\left({\mathrm{p}}_2{\mathrm{V}}_2-{\mathrm{p}}_1{\mathrm{V}}_1\right)$]