Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 2: Exercise-2

One mole of an ideal gas $\left({\mathrm{C}}_{\mathrm{v},\mathrm{m}}=\frac{5}{2}\mathrm{R}\right)$ at $300 \mathrm{K}$ and $5 \mathrm{atm}$ is expanded adiabatically to a final pressure of $2 \mathrm{atm}$, against a constant pressure of $2 \mathrm{atm}$. Final temperature of the gas is:

In Haber's process of manufacturing of ammonia:

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2{\mathrm{NH}}_3\left(\mathrm{g}\right); {\mathrm{H}}_{25°\mathrm{C}}^0=-92.2 \mathrm{kJ}$

If ${\mathrm{C}}_{\mathrm{p}}$ is independent of temperature, then reaction at $100°\mathrm{C}$ as compared to that of $25°\mathrm{C}$ will be:

The reaction of nitrogen with hydrogen to make ammonia has $\mathrm{\Delta H}=-92 \mathrm{kJ}$

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)⟶2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

What is the value of $\mathrm{\Delta U}$ (in $\mathrm{kJ}$) if the reaction is carried out at a constant pressure of $40$ bar and the volume change is $-1.25$ litre?

Calculate magnitude of $\mathrm{\Delta U}$ of the reaction in $\mathrm{kcal} {\mathrm{mol}}^{-1}$ for the hydrogenation of acetylene to ethene at constant volume and at $77°\mathrm{C}.$ Given that ${\mathrm{\Delta H}}_{\mathrm{f}}\left({\mathrm{H}}_2\mathrm{O}\right)=-67.8 \mathrm{kcal} {\mathrm{mol}}^{-1}$; ${\mathrm{\Delta H}}_{\text{comb }}\left({\mathrm{C}}_2{\mathrm{H}}_2\right)=-310.1 \mathrm{kcal} {\mathrm{mol}}^{-1}, {\mathrm{\Delta H}}_{\text{comb }}\left({\mathrm{C}}_2{\mathrm{H}}_4\right)=-337.2 \mathrm{kcal} {\mathrm{mol}}^{-1}$.

Round off your answer to the nearest integer.

Calculate the $\mathrm{C}-\mathrm{C}$ bond enthalpy from the following data:

$\left(\mathrm{a}\right) \mathrm{C}\left(\mathrm{s}\right)⟶\mathrm{C}\left(\mathrm{g}\right); \mathrm{\Delta H}=170 \mathrm{kcal}$

$\left(\mathrm{b}\right) \frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)⟶\mathrm{H}\left(\mathrm{g}\right); \mathrm{\Delta H}=52 \mathrm{kcal}$

$\left(\mathrm{c}\right)$ Heat of formation of ethane $=-20 \mathrm{kcal}$

$\left(\mathrm{d}\right) \mathrm{C}-\mathrm{H}$ bond enthalpy$=99 \mathrm{kcal}$

Which of the following is(are) endothermic reaction:

Heat of reaction depend upon:

Which of the reaction defines molar ${\mathrm{\Delta H}}_{\mathrm{f}}°?$