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:
1. \(\left(\right. \Delta U / \Delta T \left.\right){v}\)
2. \(\left(\right. \Delta H / \Delta T \left.\right)_{V}\)
3. \(\left(\right. \Delta H / \Delta T \left.\right)_{P}\)
4. \((\Delta U / \Delta T )_P\)

Plants and living beings are examples of:
1. Isolated system
2. Adiabatic system
3. Open system
4. Closed system

Find the relation between pressure and volume changes for the adiabatic expansion of an ideal gas.

What happens to a gas when it expands at constant temperature and pressure?

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 the change in internal energy is :

1. $-$200 J

2. $-$100J

3. +100J

4. + 300J

The internal energy of a substance does not depend upon:

1. Translational energy

2. Vibrational energy

3. Energy due to the gravitational pull

4. Rotational energy

Internal energy (E) and pressure of a gas of unit volume are related

as

(1) $P=\frac{2}{3}E<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$
$$

(2) $P=\frac{3}{2}E<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

(3) $<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>P=\frac{E}{2}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

(4) P=2E

Identify the false statement among the following.

Find the correct entropy condition for a spontaneous process.

1. ΔS_system + ΔS_surroundings > 0
2. ΔS_system + ΔS_surroundings < 0
3. ΔS_system > 0 only
4. ΔS_surroundings > 0 only