Which of the following statements is correct with regard to $∆$G of a cell reaction and EMF of the cell (E) in which the reaction occurs ?

(1) Both $∆$G and E are extensive properties

(2) $∆$G is an intensive property but E is an extensive property

(3) $∆$G is an extensive property and E is an intensive property

(4) Both $∆$G and E are intensive properties.

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 $∆H^{\circ }=-2.8\times {10}^6 J mo{l}^{-1}.$ [molar enthalpy of combustion]. Molar mass of glucose = 180 mol^-1.

1. $5.73\times {10}^2 J/deg$

2. $7.53\times {10}^2 J/deg$

3. $6.22\times {10}^2 J/deg$

4. $3.57\times {10}^2 J/deg$

The C-Cl bond energy can be calculated from :

1. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) only$

2. ${{∆}^{\circ }}_f\left(CC{l}_4, l\right) and ∆\left(C{l}_2\right)$

3. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) ∆\left(C{l}_2\right)$

4. $∆{H^{\circ }}_f\left(CC{l}_4, l\right) ∆\left(C{l}_2\right), ∆{H^{\circ }}_f\left(C, g\right) and ∆{H^{\circ }}_{vap}\left(CC{l}_4\right)$

Given $∆{H^{\circ }}_f$ of DyCl₃ (s) = -994.30 kJ mol^-1

$\frac{1}{2}{H}_2\left(g\right)+\frac{1}{2}C{l}_2\left(g\right)\stackrel{+aq}{\to }HCl\left(aq. 4 M\right); ∆H^{\circ }=-158.31 kJ mo{l}^{-1}$
$DyC{l}_3\left(s\right)\underset{HCl}{\overset{aq}{\to }}DyC{l}_3\left(aq. 4 M HCl\right); ∆H^{\circ }=-180.06 kJ mo{l}^{-1}$
$Dy\left(s\right)\underset{aq. 4 M}{\overset{+3 HCl}{\to }}DyC{l}_3\left(aq. 4 M HCl\right)+\frac{3}{2}{H}_2\left(g\right); ∆H^{\circ }=x, calculate x.$
$$

1. -966.5 kJ/mol

2. -699.43 kJ/mol

3. -596.6 kJ/mol

4. -569.6 kJ/mol

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

$C_P-C_V=R$. This R is :

1. Change in K.E.

2. Change in rotational energy

3. work done which system can do on expanding the gas per mol per degree increase in temperature

4. All correct