MCQ
For which of the following processes, $\Delta S$ is negative?
- A$C$ (diamond) $\to$ $C$ (graphite)
- B$N_2(g,\,1\,atm) \to N_2(g,\,5\,atm)$
- C$N_2(g,\,273\,K) \to N_2(g,\,300\,K)$
- D$H_2(g) \to 2H(g)$
✓
Answer
$(a)$ When diamond is converted into graphite when it is heated to $1500\,^oC$ and entropy is increased so $\Delta S > 0$
$(b)$ When pressure increases then molecules of gas will come closer and intermolecular distance decreases so entropy will also decrease and $\Delta S < 0$
$(c)$ When we increase the temperature of a gas then random ness is increased due to kinetic energy gained by molecules. So, $\Delta S > 0$
$(d)$ $H_2$ molecule is converted into atoms, the no. of particles increases . Thus entropy will increase. So, $\Delta S > 0$
$(b)$ When pressure increases then molecules of gas will come closer and intermolecular distance decreases so entropy will also decrease and $\Delta S < 0$
$(c)$ When we increase the temperature of a gas then random ness is increased due to kinetic energy gained by molecules. So, $\Delta S > 0$
$(d)$ $H_2$ molecule is converted into atoms, the no. of particles increases . Thus entropy will increase. So, $\Delta S > 0$
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