For the reaction, 2Cl(g) $\to$ Cl₂(g), the correct option is:

1. ${∆}_{\mathrm{r}}\mathrm{H}>0 \mathrm{and} {∆}_{\mathrm{r}}\mathrm{S}<0$

2. ${∆}_{\mathrm{r}}\mathrm{H}<0 \mathrm{and} {∆}_{\mathrm{r}}\mathrm{S}>0$

3. ${∆}_{\mathrm{r}}\mathrm{H}<0 \mathrm{and} {∆}_{\mathrm{r}}\mathrm{S}<0$

4. ${∆}_{\mathrm{r}}\mathrm{H}>0 \mathrm{and} {∆}_{\mathrm{r}}\mathrm{S}>0$

The correct option for free expansion of an ideal gas under adiabatic condition is:

1.  $q=0, ∆T<0 and w>0$

2.  $q<0, ∆T=0 and w=0$

3.  $q>0, ∆T>0 and w>0$

4.  $q=0, ∆T=0 and w=0$

The solubility of a solute in water varies with temperature and is given as $\mathrm{S}={\mathrm{Ae}}^{-∆\mathrm{H}/\mathrm{RT}}.$

Here, $∆\mathrm{H}$ is enthalpy of the solution. For the given solute variation of log, S with temperature can be shown by the figure given below.

This solute may be

1. CaSO₄ 

2. CuSO₄ 

3. CuSO₄5H₂O

5. MgO

The equilibrium constant for the reaction

${\mathrm{H}}_2\left(\mathrm{g}\right)+\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

is 18.5 at 925 and 9.25 at 1000 respectively. What is the enthalpy of the reaction?

1. -142.16 kJ/mole

2. -71.08 kJ/mole

3. -35.54 kJ/mole

4. none of these

If the value of $∆$H in a reaction is positive, then the reaction is called

(1) Exothermic

(2) Endothermic

(3) Polymorphic

(4) Polytropic

Molar heat capacity at constant P for a substance is equal to

$$\begin{gathered} \left(1\right) {(∆\mathrm{U}/∆\mathrm{T})}_{\mathrm{v}} \\ \left(2\right) {(∆\mathrm{H}/∆\mathrm{T})}_{\mathrm{V}} \\ \left(3\right) {(∆\mathrm{H}/∆\mathrm{T})}_{\mathrm{P}} \\ \left(4\right) {(∆U/∆\mathrm{T})}_{\mathrm{P}} \end{gathered}$$

Plants and living beings are examples of -

1. Isolated system.

2. Adiabatic system.

3. Open system.

4. Closed system.

For an adiabatic expansion of a perfect gas, $∆$P/P is equal to?

(1) $\frac{∆V}{V}$

(2) $-y\frac{∆V}{V}$

(3) $y\frac{∆V}{V}$

(4) $-y^2\frac{∆V}{V}$

If a gas at constant temperature and pressure expands,

then its

(1) Internal energy decreases

(2) Entropy increases and then decreases

(3) Internal energy increases

(4) Internal energy remains constant

If a gas absorbs 200 J of heat and expands by 500 ${\mathrm{cm}}^3$ against the constant pressure of

2x${10}^5$ Nm^-2 , then a change in internal energy is -

1. $-$200 J

2. $-$100J

3. +100J

4. + 300J