Thermodynamics practice · Mixed difficulty

Enthalpy of vaporisation for water is 186.5 kJ $\mathrm{mo}{\mathrm{l}^{ - 1}}$ . The entropy change during vaorisation is …kJ ${\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$ .

Which of the following is/are state function?

Assertion (A): Work is a path function which is expressed in joule.

Reason (R): Work appears only at the boundary of the system.

Statement I: Heat evolved in the neutralization of either 1 mole of ${HCl}$ or 1 mole of ${H}_2 {SO}_4$ with ${NaOH}$ is same.

Statement II: Both ${HCl}$ and ${H}_2 {SO}_4$ are strong acids.

Among the following the set of parameters that represents path functions, is
(A) $q + W\,\,\,\,\,\,\,\,\,\,$ (B) $q\,\,\,\,\,\,\,\,\,\,$ (C) $W\,\,\,\,\,\,\,\,\,\,$ (D) $H - TS$

The difference between electron gain enthalpies will be maximum between:

Identify the correct statement regarding entropy

The heat of combustion of ${CH}_{4({g})}, {C}_{(\mathrm{graphite})}$ and ${H}_{2({g})}$ are $20 \, \mathrm{kcal},-40 \, \mathrm{kcal}$ and $-10 \, \mathrm{kcal}$ respectively. The heat of formation of methane is

The entropy change for vaporisation of liquid water to steam at 100℃ is…$\mathrm{J}{\mathrm{K}^{ - 1}}\mathrm{mo}{\mathrm{l}^{ - 1}}$Given that heat of vaporisation is $40.8kJmo{l^{ - 1}}.$

Specific heat is defined as:

Calculate proton affinity of ${NH}_3(\mathrm{g})$ from the following data.

$\begin{aligned} & \Delta H_{\text {dissociation }} {H}_2=218 \mathrm{~kJ} \mathrm{~mole}^{-1} \\ & \Delta H_{\text {dissociation }} {Cl}_2=124 \mathrm{~kJ} \mathrm{~mole}^{-1} \\ & \Delta H_{\mathrm{f}}^\circ \text { of } {NH}_3(\mathrm{g})=-46 \mathrm{~kJ} \mathrm{~mole}^{-1} \\ & \Delta H_{\mathrm{f}}^\circ \text { of } {NH}_4 {Cl}(\mathrm{s})=-314 \mathrm{~kJ} \mathrm{~mole}^{-1} \end{aligned}$

Ionization energy of $H=1310 \mathrm{~kJ} \mathrm{~mole}^{-1}$

E.A. of ${Cl}(\mathrm{g})=-348 \mathrm{~kJ} \mathrm{~mole}^{-1}$

Lattice energy of ${NH}_4 {Cl}(\mathrm{s})=-683 \mathrm{~kJ} \mathrm{~mole}^{-1}$

The enthalpy of a monoatomic gas at $T$ Kelvin is:

At $25^{\circ} \mathrm{C}$ 1 mole of butane upon heating forms $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$. The work done is

The enthalpy of neutralisation of $NH_4 OH$ and $CH_3 COOH$ is $-10.5 \mathrm{k\,cal\,} \mathrm{mol}^{-1}$ and enthalpy of neutralisation of $CH_3COOH$ with strong base is $-12.5 \mathrm{k\,cal\,} \mathrm{mol}^{-1}$. The enthalpy of ionisation of $NH_4OH$ will be

For the complete combustion of ethanol, ${C_2}{H_5}OH(l) + 3{O_2}(g) \to 2C{O_2}(g) + 3{H_2}O(l),$ the amount of heat produced as measured in bomb calorimeter, is $1364.47\,k{J^{ - 1}}\,mo{l^{ - 1}}$ at $25^\circ C$. Assuming ideality the enthalpy of combustion, ${\Delta _C}H,$ for the reaction will be
($R = 8.314\,J{K^{ - 1}}\,mo{l^{ - 1}}$)

Given that $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$;
$\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-92 \mathrm{~kJ}$, the standard molar enthalpy of formation in $\mathrm{kJ} \mathrm{mol}^{-1}$ of $\mathrm{NH}_3(\mathrm{~g})$ is

Butane exists in various conformations in nature. At any given instant, the probability that a given butane molecule is in anti, gauche, eclipsed and fully eclipsed conformation is $0.7,0.2,0.06$ and $0.04 ,$ respectively. If the molar enthalpy of combustion of natural butane is $-690 \mathrm{~kcal} / \mathrm{mol}$ at $25^{\circ} \mathrm{C},$ then calculate the enthalpy of combustion of butane if all the butane molecules are in gauche conformation. The potential energy of gauche form is $2 \mathrm{~kcal} / \mathrm{mol}$ higher than anti form but it is $3 \mathrm{~kcal} / \mathrm{mol}$ less than eclipsed form and $5.5 \mathrm{~kcal} / \mathrm{mol}$ less than fully eclipsed form.

According to the first law of thermodynamics which of the following quantities represents change in a state function?

1 mol of an ideal gas expanded reversibly from 10 L to 100 L at $27^{\circ} \mathrm{C}.$ Work done involved in the process is

A process in which no heat change takes place is called.

The enthalpy changes for the following processes are listed below :

$\begin{array}{ll}\mathrm{Cl}_2(g) \rightarrow 2 \mathrm{Cl}(g), & 242.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(g) \rightarrow 2 \mathrm{I}(g), & 151.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{ICl}(g) \rightarrow \mathrm{I}(g)+\mathrm{Cl}(g), & 211.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ \mathrm{I}_2(s) \rightarrow \mathrm{I}_2(g), & 62.76 \mathrm{~kJ} \mathrm{~mol}^{-1}\end{array}$

Given that the standard states for iodine and chlorine are $\mathrm{I}_2(s)$ and $\mathrm{Cl}_2(g)$, the standard enthalpy of formation for $\operatorname{ICl}(g)$ is :

The standard heat of combustion of solid boron is :

The heat of formations of $\mathrm{CO(g})$ and $\mathrm{CO_2(g})$ are $-26.4 \mathrm{~K} \mathrm{~cal}$ and $-94.0 \mathrm{~kcal}$ respectively. The heat of combustion of carbon monoxide will be

Consider a reversible isontropic expansion of 1.0 mole of an ideal monoatomic gas from $25^{\circ} \mathrm{C}$ to $75^{\circ} \mathrm{C}$. If the initial pressure was $1.0 \mathrm{~bar}$, final pressure is

If the bond energies of $\mathrm{H}_2, \mathrm{Br}_2$ and $\mathrm{H}-\mathrm{Br}$ are 433,192 and $364 \mathrm{~kJ} /$ mol respectively the $\Delta \mathrm{H}^{\circ}$ for the reaction $\mathrm{H}_2(\mathrm{g})+\mathrm{Br}_2(\mathrm{g}) \longrightarrow 2 \mathrm{HBr}(\mathrm{g})$ is:

Which of the following on combustion gives
maximum energy?

A process which is unfavourable with respect to enthalpy,
but favourable with respect to entropy

Heat absorbed at constant volume is measured in a calorimeter in which steel vessel is immersed to ensure that

Assertion (A): The dissolution of $\mathrm{NH}_4 \mathrm{Cl}$ in water is endothermic but it dissolves in water.
Reason (R): On dissolution of $\mathrm{NH}_4 \mathrm{Cl}$, entropy increases.

The molar heat capacity, $\mathrm{C}_{\mathrm{v}}$ of an ideal gas whose energy is that of translational motion only is