Thermodynamics

Calculate $\Delta \mathrm{S}_{\text {Iotal }}$ for a certain reaction if $\Delta \mathrm{H}=-150 \mathrm{~kJ}$ and $\Delta \mathrm{S}=32 \mathrm{JK}^{-1}$ at 300 K .

Calculate the change in internal energy of the system if work done by the system is 18 joule and absorbs heat 50 joule in a particular reaction.

Identify from following the correct set of thermodynamic conditions for a reaction to be nonspontaneous at all temperatures.

Identify from following the correct set of thermodynamic conditions for the reaction to be spontaneous at all temperature.

Calculate the work done if 1 mole of certain gas compressed isothermally and reversibly at 300 K from initial pressure $x$ bar to final pressure $2 x$ bar $\left[\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

Calculate the standard enthalpy change of following reaction.
$$ \begin{aligned} & \mathrm{CH}_{4(\mathrm{~s})}+2 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\ell)} \\ & \text { if } \Del...

Calculate the work done in joule if 1 mole of ideal gas is compressed from $25 \mathrm{dm}^3$ to $13 \mathrm{dm}^3$ at constant external pressure 4 bar.

Which from following transformations is endothermic in nature?

Calculate $\Delta \mathrm{H}^{\circ}$ for a reaction if $\Delta \mathrm{S}^{\circ}=120 \mathrm{JK}^{-1}$ and $\Delta \mathrm{G}^{\circ}=28000 \mathrm{~J}$

Which from following is an example of both intensive property and state function?

Calculate the work done in joule if 1 mole of an ideal gas compressed from volume $24 \mathrm{dm}^3$ to $13 \mathrm{dm}^3$ at constant external pressure 3 bar.

For a certain reaction, $\Delta \mathrm{H}=-210 \mathrm{~kJ}$ and $\Delta \mathrm{S}=-150 \mathrm{~kJ} \mathrm{~K}^{-1}$ Find the temperature so that $\Delta \mathrm{G}=0$.

Which from following reactions is exothermic?

Calculate the standard enthalpy change for reaction,
$$ \begin{aligned} & \mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}_{(l)}+3 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+3 \mathrm{H}_2 \mathrm{O}_{(l)} \\ & \text { ...

Calculate work done in isothermal reversible expansion of 1 mole ideal gas from initial pressure 10 bar to final pressure 1 bar at 300 K . $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$.

Calculate work done if 1 mole of an ideal gas expands isothermally from $2 \mathrm{dm}^3$ to $2.8 \mathrm{dm}^3$ against constant external pressure 1 atm .

Identify from following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.

Calculate the standard enthalpy change for synthesis of ammonia gas from following data.
i. $\quad 2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{N}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_2 \mathrm{H}_{4(\mathrm{~g})} ; \Delta_{\mathrm{r}} \mat...

1.8 g water is vapourised by supplying 4 kJ heat at $100^{\circ} \mathrm{C}$. What is the heat of vapourisation of water at same temperature?

Calculate the standard enthalpy change of following reaction
$$ \begin{aligned} & \mathrm{CH}_{4(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\ell)} \\ & \text { If } \Delt...

Calculate the work done in joule if 2 moles of an ideal gas expand isothermally from $15.5 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at constant pressure 1 atm .

Calculate the change in internal energy of the system if 20 kJ work is done on the system and it releases 10 kJ heat in a particular reaction.

Calculate the enthalpy of solution of potassium chloride if its $\Delta_{\mathrm{L}} \mathrm{H}=700 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta_{\text {hyd }} H=-680 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Identify from following reactions that exhibits negative work done.

Find standard enthalpy of formation of ammonia from following reaction.
\(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})} ; \Delta_{\mathrm{r}} \mathrm{H}^0=-92.0 \mathrm{~kJ}\)

Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?

Calculate the work done in following reaction at $27^{\circ} \mathrm{C}$.
$$ \begin{aligned} & 4 \mathrm{SO}_{2(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{SO}_{3(\mathrm{~g})} \\ & \left(\mathrm{R}=8.314 \mathrm{~...

Calculate standard enthalpy change of reaction
\(\mathrm{C}_2 \mathrm{H}_{2(\mathrm{~g})}+\frac{5}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}, \text { if }\)
$$ \be...

Identify from following an example of intensive property?

Calculate the change in internal energy of the system if 25 kJ of work done by the system and it absorbs 10 kJ of heat.

Calculate the enthalpy of vaporisation of ethanol if 11.5 g of ethanol is completely vaporised by supplying 11.8 kJ of heat.

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

Which from following process involves zero work done?

Identify from following physical transformations that exhibits decrease in entropy.

Calculate the standard enthalpy change of following reaction.
\(\mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+3 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(l)}\)
If $\Delta_{\mathrm{f}...

Calculate work done if 1 mole of an ideal gas compressed isothermally and reversibly from 12 $\mathrm{dm}^3$ to $6 \mathrm{dm}^3$ at $300 \mathrm{~K} .\left[\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right]$

Calculate $\Delta \mathrm{S}_{\text {total }}$ for a certain reaction at 298 K if $\Delta \mathrm{H}^{\circ}=-208.6 \mathrm{~kJ}$ and $\Delta \mathrm{S}^{\circ}=-36 \mathrm{~J} \mathrm{~K}^{-1}$

Which from following reactions performs zero work?

Calculate the change in internal energy of the system if 20 kJ of work is done on the system and it releases 10 kJ of heat in a particular reaction.

Which of the following reactions exhibits decrease in entropy?

Calculate the enthalpy change of vaporisation of benzene if 13 gram of benzene vaporised by supplying 5.1 kJ of heat.

Calculate the entropy change of surrounding if 2 moles of $\mathrm{H}_2$ and 1 mole of $\mathrm{O}_2$ gas combine to form 2 moles of liquid water by releasing 525 kJ heat to surrounding at constant pressure and at 300 K .

Two moles of an ideal gas is expanded isothermally from a volume of $300 \mathrm{~cm}^3$ to 2.5 $\mathrm{dm}^3$ at 298 K against a constant pressure at 1.9 bar. Calculate the work done in joules.

What is change in internal energy of the system when work done by the system is 150 J and system release 300 J of heat?

For the reaction,
\(\mathrm{C}_3 \mathrm{H}_{8(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 3 \mathrm{CO}_{2(\mathrm{~g})}+4 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}\)
at constant temperature, $\Delta \mathrm{H}-\Delta \mathrm{...

For the reaction,
\(2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}, \Delta \mathrm{H}^{\circ}=-573.2 \mathrm{~kJ}\)
What is heat of decomposition of water per mol?

10 g each of $\mathrm{NH}_3, \mathrm{~N}_2, \mathrm{Cl}_2$ and $\mathrm{H}_2 \mathrm{~S}$ are expanded isothermally and reversibly at same temperature. Identify gas that performs maximum work.

Identify the factor from following on which heat of reaction does not depend.

Which of the following set of properties is correct when one mole of a gas is heated keeping volume constant by increasing temperature and supplying 500 J of heat?

Calculate the entropy change for melting 1 g ice at $0^{\circ} \mathrm{C}$ in $\mathrm{Jg}^{-1} \mathrm{~K}^{-1}$ if heat of fusion of ice at $0^{\circ} \mathrm{C}$ is $80 \mathrm{~J} \mathrm{~K}^{-1}$.