Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 1: AMU-AT (B.Tech.) 2017

Calculation the maximum work done in expanding $16 \mathrm{g}$of oxygen at $300 \mathrm{K}$ and occupying a volume of $5 {\mathrm{dm}}^3$ isothermally until volume becomes $25 {\mathrm{dm}}^3$.

For the reaction,

$\frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$

${\mathrm{\Delta G}}_{\text{recation }}°=-131.23 \mathrm{kJ} {\mathrm{mol}}^{-1}$

The value of ${\mathrm{\Delta G}}_{\text{formation }}°$ of ${\mathrm{Ag}}^{+}$ (aq) shall be given by, (if ${\mathrm{\Delta G}}_{\mathrm{f}}°\left({\mathrm{H}}^{+}\mathrm{aq}\right)=0$)

A better criterion for ideality of a gas than ${\left(\frac{\partial \mathrm{U}}{\partial \mathrm{V}}\right)}_{\mathrm{T}}=0$ is

An ideal gas initially at temperature, pressure and volume, $27°\mathrm{C},1.00$ bar and $10 \mathrm{L}$ respectively is heated at constant volume until pressure is $10.0$ bar, it then undergoes a reversible isothermal expansion until pressure is $1.00\mathrm{bar},$ what is the total work $\mathrm{W}$, during this process?

For the reaction, ${\mathrm{S}}_{\text{(rhombic) }}+{\mathrm{O}}_2\to {\mathrm{SO}}_2$ $\mathrm{\Delta H}=-298 \mathrm{kJ} {\mathrm{mol}}^{-1}$  at $25°\mathrm{C}$ and $1 \mathrm{atm}$. Therefore, $\Delta E$ for the reaction should be

The difference between ${\overline{\mathrm{C}}}_{\mathrm{p}}$ and ${\overline{\mathrm{C}}}_{\mathrm{V}}$ is $\left[{\overline{\mathrm{C}}}_{\mathrm{p}}\right.$ and ${\overline{\mathrm{C}}}_{\mathrm{V}}$ signify molar quantities]

A gas can expand from $100 \mathrm{mL}$ to $250 \mathrm{mL}$ under a constant pressure of $2 \mathrm{atm}$. The work done by gas is

Hess law states that,