Melting point of a solid is $x \ K$ and its latent heat of fusion is $600 \ cal \ mol^{-1}$. The entropy change for fusion of $1 \ mol$ solid is $2 \ cal \ mol^{-1} \ K^{-1}$. The value of $x$ will be......$K$

Ice at $-5^{\circ} C$ is heated to become vapor with a temperature of $110^{\circ} C$ at atmospheric pressure. The entropy change associated with this process can be obtained from:

When $2 \ mol$ of an ideal gas $\left( C_{p,m} = \frac{5}{2} R \right)$ is heated from $300 \ K$ to $600 \ K$ at constant pressure,the change in entropy of the gas $\left( \Delta S \right)$ is:

Amongst the chemical reactions given below, the reactions with increasing entropy are
$(i)$ $H_2O_{(l)} \rightarrow H_2O_{(g)}$
$(ii)$ $C_{(s)} + CO_{2(g)} \rightarrow 2CO_{(g)}$
$(iii)$ $2H_{2(g)} + O_{2(g)} \rightarrow 2H_2O_{(l)}$
$(iv)$ $N_{2(g)} + O_{2(g)} \rightarrow \text{Mixture of } N_2 \text{ and } O_2$

The entropy change when $2 \, \text{moles}$ of an ideal monoatomic gas is heated from $200 \, ^\circ \text{C}$ to $300 \, ^\circ \text{C}$ isochorically is:

Which of the following processes is associated with a decrease in entropy?