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Following data is known about melting of a compound AB. $∆\mathrm{H}=9.2 \mathrm{kJ} {\mathrm{mol}}^{-1}, ∆\mathrm{S}=0.008 {\mathrm{kJK}}^{-1}{\mathrm{mol}}^{-1}$. Its melting point is:
(1) 736 K
(2) 1050 K
(3) 1150 K
(4) 1150$°$C

Which of the following conditions will always lead to a non-spontaneous change?
1. Positive $∆H$ and positive $∆S$
2. Negative$∆H$ and negative $∆S$
3. Positive $∆H$ and negative $∆S$
4. Negative $∆H$ and positive $∆P$

To calculate the amount of work done in joules during reversible isothermal expansion of an ideal gas, the volume must be expressed in:

For the conversion C_(graphite) $\to$C_(diamond) the $∆S$ is:
1. Zero
2. Positive
3. Negative
4. Unknown

The entropy change in the conversion of one mole of liquid water at 373 K to vapour at the same temperature would be: (Latent heat of vaporization of water, $∆H_{vap}=2.257$ $kJ/g$)
1. 105.9 JK^-1mol^-1
2. 107.9 JK^-1mol^-1
3. 108.9 JK^-1mol^-1
4. 109.9 JK^-1mol^-1

\(\underset {-10.7 \mathrm{JK}^{-1}} {\mathrm{H}_{(a q)}^{+}+\mathrm{OH^{-}}_{(a q)}} \rightarrow \underset {+70 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} } {\mathrm{H}_{2} \mathrm{O}_{(l)}} ~~ \mathrm{S}^{\circ}(298 \mathrm{~K})\)
Standard entropy change for the above reaction is:
1. 60.3 JK^-1 mol^-1
2. 80.7 JK^-1 mol^-1
3. -70 JK^-1 mol^-1
4. +10.7 JK^-1 mol^-1

Standard entropies of ${\mathrm{X}}_2, {\mathrm{Y}}_2 \mathrm{and} {\mathrm{XY}}_3$ are 60, 40 and 50 JK^-1 mol^-1 respectively. For the reaction
$\frac{1}{2}{X}_2+\frac{3}{2}{Y}_2\rightleftharpoons X{Y}_3, ∆H=-30 kJ$
to be at equilibrium, the temperature should be:
(1) 500 K
(2) 750 K
(3) 1000 K
(4) 1250 K

A gas $\left({\mathrm{C}}_{\mathrm{v},\mathrm{m}}=\frac{5}{2}\mathrm{R}\right)$ behaving ideally was allowed to expand reversibly and adiabatically from 1 litre to 32 litre. Its initial temperature was 327$°C$. The molar enthalpy change  (in J/mol) for the process is:
(1) -1125 R
(2) -675
(3) -1575 R
(4) None of these

Two mole of an ideal gas is heated at constant pressure of one atmosphere from $27°\mathrm{C} \mathrm{to} 127°\mathrm{C}$. If ${\mathrm{C}}_{\mathrm{v}.\mathrm{m}}=20+{10}^{-2} \mathrm{T} {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$, q and $∆U$ for the process are respectively:
(1) 6362.8 J, 4700 J
(2) 3037.2 J, 4700 J
(3) 7062.8 J, 5400 J
(4) 3181.4 J, 2350 J

2 mole of an ideal monoatomic gas undergoes a reversible process for which ${\mathrm{PV}}^2=\mathrm{C}$. The gas is expanded from initial volume of 1 L to final volume of 3 K starting from initial temperature of 300 K. Find $∆\mathrm{H}$ for the process:
(1) -600 R
(2) -1000 R
(3) -3000 R
(4) None of these

Calculate $∆S$ for 3 mole of a diatomic ideal gas which is heated and compressed from 298 K and 1 bar to 596 K and 4 bar: [${\mathrm{C}}_{\mathrm{v},\mathrm{m}}\left(\mathrm{gas}\right)=\frac{5}{2}\mathrm{R}; \mathrm{Ln}\left(2\right)=0.70;\mathrm{R}=2 \mathrm{cal} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-2}$]
(1) $-14.7 \mathrm{cal} {\mathrm{K}}^{-1}$
(2) $+14.7 \mathrm{cal} {\mathrm{K}}^{-1}$
(3) $-14.9 \mathrm{cal} {\mathrm{K}}^{-1}$
(4) $6.3 \mathrm{cal} {\mathrm{K}}^{-1}$

Two mole of an ideal gas is expanded irreversibly and isothermally at $37°\mathrm{C}$ until its volume doubled and 3.41 kJ heat is absorbed from surrounding. $∆{\mathrm{S}}_{\mathrm{total}}$(System+surrounding) is 
(1) -0.52 J/K
(2) 0.52 J/K
(3) 22.52 J/K
(4) 0

For a perfectly crystalline solid $C_{p,m}=a{T}^3+bT$, where a and b are constant. If ${\mathrm{C}}_{\mathrm{p},\mathrm{m}}$ is 0.47 J/K mol at 10 K and 0.92 J/K mol at 20 K, then molar entropy at 20 K is:
(1) 0.92 J/K mol
(2) 8.66 J/K mol
(3) 0.813 J/K mol
(4) None of these

Calculate ${∆}_{\mathrm{f}}\mathrm{H}°$ (in kJ/mol) for ${\mathrm{Cr}}_2{\mathrm{O}}_3$ from the ${∆}_{\mathrm{r}}\mathrm{G}° \mathrm{and} \mathrm{the} \mathrm{S}°$ values provided at $27°\mathrm{C}$
$4\mathrm{Cr}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{Cr}}_2{\mathrm{O}}_3\left(\mathrm{s}\right); {∆}_{\mathrm{r}}\mathrm{G}°=-2093.4 \mathrm{kJ}/\mathrm{mol}$
$\mathrm{S}° (\mathrm{J}/\mathrm{K} \mathrm{mol}): \mathrm{S}° (\mathrm{Cr},\mathrm{s})=24; \mathrm{S}°({\mathrm{O}}_2,\mathrm{g})=205; \mathrm{S}°({\mathrm{Cr}}_2{\mathrm{O}}_3,\mathrm{s})=81$
(1) -2258.1 kJ/mol
(2) -1129.05 kJ/mol
(3) -964.35 kJ/mol
(4) None of these

Calculate the heat produced (in kJ) when 224 gm of CaO is completely converted to ${\mathrm{CaCO}}_2$ by reaction with ${\mathrm{CO}}_2 \mathrm{at} 27°\mathrm{C}$ in a container of fixed volume.
$\mathrm{Given}: ∆\mathrm{H}{°}_{\mathrm{f}}({\mathrm{CaCO}}_3,\mathrm{s})=-1207 \mathrm{kJ}/\mathrm{mol}; ∆{\mathrm{H}}_{\mathrm{f}}^{°}(\mathrm{CaO},\mathrm{s})=-635 \mathrm{kJ}/\mathrm{mol}$
$∆{\mathrm{H}}_{\mathrm{f}}^{°}({\mathrm{CO}}_2,\mathrm{g})=-394 \mathrm{kJ}/\mathrm{mol}; [\mathrm{Use} \mathrm{R}=8.3 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}]$
(1) 702.04 kJ
(2) 721.96 kJ
(3) 712 kJ
(4) 721 kJ

When 1.- g of oxalic acid $\left({\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4\right)$ is burned in a bomb calorimeter whose heat capacity is 8.75 kJ/K, the temperature increases by 0.312 K. The enthalpy of combustion of oxalic acid is $27°C$
(1) -245.7 kJ/mol
(2) -244.452 kJ/mol
(3) -241.5 kJ/mol
(4) None of these

Enthalpy of neutralization of ${\mathrm{H}}_3{\mathrm{PO}}_3$ acid is -106.69 kJ/mol using NaOH. Enthalpy of neutralization of HCl by NaOH is -55.84 kJ/mol. $∆{\mathrm{H}}_{\mathrm{ionization}} \mathrm{of} {\mathrm{H}}_3{\mathrm{PO}}_3$ is -
1. 50.84 kJ/mol
2. 5 kJ/mol
3. 2.5 kJ/mol
4. None of these

The enthalpy of neutralization of a weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 kJ/mol. If the unionized acid required 1.4 kJ/mol heat for its complete ionization and enthalpy of neutralization of the strong monobasic acid with a strong monoacidic base is -57.3 kJ/mol, what is the % ionization of the weak acid in molar solution
1. 1%
2. 3.57 %
3. 35.7%
4. 10%

Determine C-C and C-H bond enthalpy (in kJ/mol)
$\mathrm{Given}: {∆}_{\mathrm{f}}\mathrm{H}°({\mathrm{C}}_2{\mathrm{H}}_6, \mathrm{g})=-85 \mathrm{kJ}/\mathrm{mol},$
${∆}_{\mathrm{f}}\mathrm{H}°({\mathrm{C}}_3{\mathrm{H}}_8,\mathrm{g})=-104 \mathrm{kJ}/\mathrm{mol}$
${∆}_{\mathrm{sub}}\mathrm{H}°(\mathrm{C},\mathrm{s})=718 \mathrm{kJ}/\mathrm{mol},$
$\mathrm{B}.\mathrm{E}.(\mathrm{H}-\mathrm{H})=436 \mathrm{kJ}/\mathrm{mol}$
(1) 414, 345
(2) 345, 414
(3) 287, 404.5
(4) None of these

Consider the following data:
 ${∆}_{\mathrm{f}}\mathrm{H}°({\mathrm{N}}_2{\mathrm{H}}_4,\mathrm{l})=50 \mathrm{kJ}/\mathrm{mol}, {∆}_{\mathrm{f}}\mathrm{H}°({\mathrm{NH}}_3,\mathrm{g})=-46 \mathrm{kJ}/\mathrm{mol}$
$\mathrm{B}.\mathrm{E} (\mathrm{N}-\mathrm{H})=393 \mathrm{kJ}/\mathrm{mol} \mathrm{and} \mathrm{B}.\mathrm{E} (\mathrm{H}-\mathrm{H})=436 \mathrm{kJ}/\mathrm{mol}$
${∆}_{\mathrm{vap}}\mathrm{H}({\mathrm{N}}_2{\mathrm{H}}_4,\mathrm{l})=18 \mathrm{kJ}/\mathrm{mol}$
The N-N bond energy is ${\mathrm{N}}_2{\mathrm{H}}_4$ is:
(1) 226 kJ/mol
(2) 154 kJ/mol
(3) 190 kJ/mol
(4) None of these