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Which among the following state functions is an extensive property of the system?

Which, among the following, is not a state function?
1. Internal energy
2. Free energy
3. Work
4. Enthalpy

Given that
${\mathrm{CH}}_4\left(\mathrm{g}\right)+360<mspace\; width="1em"></mspace>\mathrm{kJ}\to \mathrm{C}\left(\mathrm{g}\right)+4\mathrm{H}\left(\mathrm{g}\right)$
${\mathrm{C}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)+620<mspace\; width="1em"></mspace>\mathrm{kJ}\to 2\mathrm{C}\left(\mathrm{g}\right)+6\mathrm{H}\left(\mathrm{g}\right)$
The value of C-C bond energy is
1. 260 kJ mol^-1
2. 180 kJ mol^-1
3. 130 kJ mol^-1
4. 80 kJ mol^-1

The work done on the system when one mole of an ideal gas at 500 K is compressed isothermally and reversibly to 1/10th of its original volume (R = 2 cal)
1. 500 kcal
2. 1.51 kcal
3. -23.30 kcal
4. 2.303 kcal

For the process
${\mathrm{NH}}_3\left(\mathrm{g}\right)+\mathrm{HCl}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\to {\mathrm{NH}}_4\mathrm{Cl}\left(\mathrm{s}\right)$
1. Both $∆\mathrm{H}$ and $∆\mathrm{S}$ are +ve 
2. $∆\mathrm{H}$ is -ve and $∆\mathrm{S}$ is +ve
3. $∆\mathrm{H}$ is +ve and $∆\mathrm{S}$ is -ve
4. Both $∆\mathrm{H}$ and $∆\mathrm{S}$ are -ve

Two moles of an ideal gas is heated at a constant pressure of one atmosphere from 27$°$C to 127$°$C. If ${\mathrm{C}}_{\mathrm{v},<mspace\; width="1em"></mspace>\mathrm{m}}=20+{10}^{-2}<mspace\; width="1em"></mspace>\mathrm{T}<mspace\; width="1em"></mspace>{\mathrm{JK}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1},<mspace\; width="1em"></mspace>$ then q and $△\mathrm{U}$ 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

Calculate ${△}_{\mathrm{f}}{\mathrm{G}}^{\circ }$ for $\left({\mathrm{NH}}_4\mathrm{Cl},<mspace\; width="1em"></mspace>\mathrm{s}\right)$ at 310 K.
Given : ${△}_{\mathrm{f}}{\mathrm{H}}^{\circ }<mspace\; width="1em"></mspace>\left({\mathrm{NH}}_4\mathrm{Cl},<mspace\; width="1em"></mspace>\mathrm{s}\right)=-314<mspace\; width="1em"></mspace>\mathrm{kJ}/\mathrm{mol};<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>{△}_{\mathrm{r}}{\mathrm{C}}_{\mathrm{p}}=0$
${\mathrm{S}}^{\circ }{\mathrm{N}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)=192<mspace\; width="1em"></mspace>{\mathrm{JK}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1};<mspace\; width="1em"></mspace>{\mathrm{S}}^{\circ }{\mathrm{H}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)=130.5<mspace\; width="1em"></mspace>{\mathrm{JK}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1};$
${\mathrm{S}}^{\circ }{\mathrm{Cl}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)=233<mspace\; width="1em"></mspace>{\mathrm{JK}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1};<mspace\; width="1em"></mspace>{\mathrm{S}}^{\circ }{\mathrm{NH}}_4\mathrm{Cl}<mspace\; width="1em"></mspace>\left(\mathrm{s}\right)=99.5<mspace\; width="1em"></mspace>{\mathrm{JK}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}$
All given data at 300 K.
1.  –198.56 kJ/mol
2.  –426.7 kJ/mol
3.  –202.3 kJ/mol
4.  None of these

Determine $△{\mathrm{U}}^{\circ }$ at 300 K for the following reaction using the listed enthalpies of reaction:
$\begin{array}{ccc}4\mathrm{CO}\left(\mathrm{g}\right)+8{\mathrm{H}}_2\left(\mathrm{g}\right)& \to & 3{\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\\ \mathrm{C}\left(\mathrm{graphite}\right)+1/2<mspace\; width="1em"></mspace>{\mathrm{O}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)& \to & \mathrm{CO}\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>△{{\mathrm{H}}_1}^{\circ }=-110.5<mspace\; width="1em"></mspace>\mathrm{kJ}\\ \mathrm{CO}\left(\mathrm{g}\right)+1/2<mspace\; width="1em"></mspace>{\mathrm{O}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)& \to & {\mathrm{CO}}_2\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>△{{\mathrm{H}}_2}^{\circ }=-282.9<mspace\; width="1em"></mspace>\mathrm{kJ}\\ {\mathrm{H}}_2\left(\mathrm{g}\right)+1/2<mspace\; width="1em"></mspace>{\mathrm{O}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)& \to & {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right);<mspace\; width="1em"></mspace>△{{\mathrm{H}}_3}^{\circ }=-285.8<mspace\; width="1em"></mspace>\mathrm{kJ}\\ \mathrm{C}\left(\mathrm{graphite}\right)+2{\mathrm{H}}_2<mspace\; width="1em"></mspace>\left(\mathrm{g}\right)& \to & {\mathrm{CH}}_4\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>△{{\mathrm{H}}_4}^{\circ }=-74.8<mspace\; width="1em"></mspace>\mathrm{kJ}\end{array}$
1.  -653.5 kJ
2.  -686.2 kJ
3.  -747.4 kJ
4.  None of these

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

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

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

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. $∆{\mathrm{H}}_{\mathrm{ionization}}<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>{\mathrm{H}}_3{\mathrm{PO}}_3$ is -
1. 50.84 kJ/mol
2. 5 kJ/mol
3. 2.5 kJ/mol
4. None of these