Embibe Experts Solutions for Chapter: Thermodynamics, Exercise 1: AP EAPCET 2020 (24-Sep Shift-1)

A system undergoes a process in which $\mathrm{\Delta U}=+300 \mathrm{J}$ while absorbing $400 \mathrm{J}$ of heat energy and undergoing an expansion against $0.5$ bar. What is the change in volume (in $\mathrm{L}) ?$

When a gas is allowed to expand in a well-insulated container, against a constant external pressure of $5$ atm, from an initial value of $10 \mathrm{L}$ to a final volume of $15 \mathrm{L},$ find the change in the internal energy $\left(\mathrm{\Delta U}\right)$ of the gas.

Given that a person inhales $640 \mathrm{g}$ of oxygen per day, assuming all the inhaled ${\mathrm{O}}_2$ is utilized in converting sugar (sucrose) to ${\mathrm{CO}}_2$ and ${\mathrm{H}}_2\mathrm{O}.$ Find the amount of heat evolved. [${\mathrm{\Delta H}}_{\text{combustion }}$ of sucrose is $-5645 \mathrm{kJ}.{\mathrm{mol}}^{-1}$]

Find the $\mathrm{\Delta H}°$ for the reaction ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}+{{\mathrm{Br}}_2}_{\left(\mathrm{g}\right)}⟶{\mathrm{HBr}}_{\left(\mathrm{g}\right)}+{\mathrm{HOBr}}_{\left(\mathrm{g}\right)}$ using:
Bond energy of $\mathrm{O}-\mathrm{H}$ bond in Water $=463 \mathrm{kJ}$
Bond energy of $\mathrm{Br}-\mathrm{Br}$ bond in ${\mathrm{Br}}_2=192 \mathrm{kJ}$
Bond energy of $\mathrm{O}-\mathrm{Br}$ bond in $\mathrm{HOBr}=234 \mathrm{kJ}$
Bond energy of $\mathrm{H}-\mathrm{Br}$ bond in $\mathrm{HBr}=364 \mathrm{kJ}$

If the enthalpy of combustion of ${\mathrm{CH}}_4$ and ${\mathrm{CH}}_3\mathrm{OH}$ are $\text{'}\mathrm{x}\text{'}$ and $\text{'}\mathrm{y}\text{'}$ respectively, then find the enthalpy of the reaction ${\mathrm{CH}}_4+\frac{1}{2}{\mathrm{O}}_2⟶{\mathrm{CH}}_3\mathrm{OH}$

The formation of an oxide ion from Oxygen atom takes place as shown below. This two-step process is unfavourable, even though ${\mathrm{O}}^{2-}$ is iso-electronic with Neon, due to the fact that

${\mathrm{O}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}⟶{\mathrm{O}}_{\left(\mathrm{g}\right)}^{-}; {\mathrm{\Delta H}}_{\mathrm{f}}°=-141 \mathrm{kJ}.{\mathrm{mol}}^{-1}$

${\mathrm{O}}_{\left(\mathrm{g}\right)}^{-}+{\mathrm{e}}^{-}⟶{\mathrm{O}}_{\left(\mathrm{g}\right)}^{2-};{\mathrm{\Delta H}}_{\mathrm{f}}^0=+780 \mathrm{kJ}.{\mathrm{mol}}^{-1}$

What would be the equilibrium temperature of the reaction $\mathrm{CO}+\frac{1}{2}{\mathrm{O}}_2⟶{\mathrm{CO}}_2,$ given that the enthalpy and entropy changes of this reaction are $-285.4 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ and $-0.94 \mathrm{kJ}{ \mathrm{mol}}^{-1}{ \mathrm{K}}^{-1}$ respectively.

A certain reaction, for which the enthalpy change is $24.85 \mathrm{kJ},$ is at equilibrium at $82°\mathrm{C}.$ Find the value of $∆\mathrm{S}$ for this reaction.