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

(1) $\frac{∆V}{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

(2) $<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>-y\frac{∆V}{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

(3) $<mspace\; width="1em"></mspace>y\frac{∆V}{V}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>$

(4) $<mspace\; width="1em"></mspace>-y^2\frac{∆V}{V}<mspace\; width="1em"></mspace>$

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.

Considering entropy (S) as a thermodynamic parameter, the criterion for the spontaneity of any process is:


1. $∆S_{system}+∆S_{surroundings}>0$

2. $∆S_{system}-∆S_{surroundings}>0$

3. $∆S_{system}>\mathrm{0\; only}$

4. $∆S_{s\mathrm{urroundings}}>\mathrm{0\; only}$

For which of the following processes will the entropy increase?

Which of the following is the correct first law thermodynamics equation?

(1) $U=∆Q-W$
$$

(2) $∆W=∆U+∆Q$
$$

(3) $∆U=∆W+∆Q$

(4) None of the above 

Which of the following conditions result in a spontaneous reaction?

1. Exothermic and increasing disorder

2. Exothermic and decreasing disorder

3. Endothermic and increasing disorder

4. Endothermic and decreasing disorder