Temperature of 1 mol of a gas is increased by $1^{\circ }$ at constant pressure. Work done is-

1. -R

2. 2R

3. R/2

4. 3R

When 0.16 g of glucose was burnt in a bomb calorimeter, the temperature rose by 4 deg. Calculate the calorimeter constant (water equivalent of the calorimeter) given that $∆H^{\circ }=-2.8\times {10}^6<mspace\; width="1em"></mspace>J<mspace\; width="1em"></mspace>mo{l}^{-1}.$ [molar enthalpy of combustion]. Molar mass of glucose = 180 mol^-1.

1. $5.73\times {10}^2<mspace\; width="1em"></mspace>J/deg$

2. $7.53\times {10}^2<mspace\; width="1em"></mspace>J/deg$

3. $6.22\times {10}^2<mspace\; width="1em"></mspace>J/deg$

4. $3.57\times {10}^2<mspace\; width="1em"></mspace>J/deg$

The C-Cl bond energy can be calculated from :

1. $∆{H^{\circ }}_f\left(CC{l}_4,<mspace\; width="1em"></mspace>l\right)<mspace\; width="1em"></mspace>only$

2. ${{∆}^{\circ }}_f\left(CC{l}_4,<mspace\; width="1em"></mspace>l\right)<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>∆\left(C{l}_2\right)$

3. $∆{H^{\circ }}_f\left(CC{l}_4,<mspace\; width="1em"></mspace>l\right)<mspace\; width="1em"></mspace>∆\left(C{l}_2\right)$

4. $∆{H^{\circ }}_f\left(CC{l}_4,<mspace\; width="1em"></mspace>l\right)<mspace\; width="1em"></mspace>∆\left(C{l}_2\right),<mspace\; width="1em"></mspace>∆{H^{\circ }}_f\left(C,<mspace\; width="1em"></mspace>g\right)<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>∆{H^{\circ }}_{vap}\left(CC{l}_4\right)$

Consider the following thermochemical data at standard conditions where enthalpy values are in\(\text{ kJ mol}^{-1}\): 

Using Hess's Law, calculate the value of \(\Delta H^\circ\) (in \(\text{kJ mol}^{-1}\)) for the following reaction;

When 1 g H₂ gas at S.T.P is expanded to twice its initial volume, then the work done is:

1. 22.4 L atm
2. 5.6 L atm
3. 11.2 L atm
4. 44.8 L atm

The gas absorbs 100 J heat and is simultaneously compressed by a constant external pressure of 1.50 atm from 8 lit. to 2 lit. in volume. Hence $∆E$ will be-

1. -812 J

2. 812 J

3. 1011 J

4. 911 J

If $∆G=∆H-T∆S$ and $∆G=∆H+T{\left(\frac{d\left(∆G\right)}{dT}\right)}_P$ then variation of EMF of a cell E, with temperature T, is given by

1. $\frac{∆H}{nF}$ 

2. $\frac{∆G}{nF}$

3. $\frac{∆S}{nF}$

4. $-\frac{∆S}{nF}$

The standard heat of combustion of Al is -837.8 kJ mol^-1 at ${25}^{\circ }C$ which of the following releases 250 kcal of heat ?

1. The reaction of 0.624 mol of Al

2. The formation of 0.624 mol of Al₂O₃

3. The reaction of 0.312 mol of Al

4. The formation of 0.150 mol of Al₂O₃

Which of the following statements correctly represents the physical meaning
of the gas constant R in the relation Cp − Cv = R?

1. It represents the change in kinetic energy of the gas.

2. It represents the change in rotational energy of the gas molecules.

3. It represents the work done by an ideal gas per mole per kelvin during expansion

4. All of the above are correct.

Heat of neutralisation of oxalic acid is -25.4 K cal mol^-1 using strong base, NaOH. Hence enthalpy change of the process is $H_2{C}_2{O}_4\rightleftharpoons 2H^{+}+C_2{H_4}^{2-}<mspace\; width="1em"></mspace>$is-

1. 2.0 kcal

2. -11.8 kcal

3. 1.0 kcal

4. -1.0 kcal