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(B) Entropy $(S)$ is a measure of the randomness or disorder of a system. Processes that lead to a more ordered state result in a decrease in entropy

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Crystallisation of a liquid into a solid

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(B) Entropy $(S)$ is a measure of the randomness or disorder of a system. Processes that lead to a more ordered state result in a decrease in entropy $(\Delta S $(A)$ Raising the temperature of a solid increases the vibrational motion of particles,leading to an increase in entropy. $(B)$ Crystallisation of a liquid into a solid involves the transition from a disordered liquid state to a highly ordered crystalline solid state,which results in a decrease in entropy. $(C)$ The decomposition of $2NaHCO_{3(s)}$ produces gaseous products ($CO_2$ and $H_2O$),which significantly increases the disorder of the system. $(D)$ The dissociation of $H_{2(g)}$ into $2H_{(g)}$ increases the number of particles and the randomness of the system,leading to an increase in entropy. Therefore,the correct option is $B$.

$a$. Liquid to vapor conversion	$1$. $\Delta S = 0$
$b$. Reaction not spontaneous at any temperature,$\Delta H = (+)$	$2$. $\Delta S = (+)$
$c$. Reversible expansion of an ideal gas	$3$. $\Delta S = (-)$

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

Similar Questions

The enthalpy change for the transition of liquid water to steam,$\Delta H_{vap} = 37.3 \ kJ \ mol^{-1}$ at $373 \ K$. The entropy change for the process is......$J \ mol^{-1} K^{-1}$.

The entropy change for the conversion of $1 \, \text{mol}$ of liquid water to steam at $373 \, K$ is ...... $J/K$ (Given: $\Delta H_{\text{vap}} = 2.257 \, kJ/g$). (in $0.9$)

Match the following processes with their corresponding entropy changes:
$a$. Liquid to vapor conversion $1$. $\Delta S = 0$
$b$. Reaction not spontaneous at any temperature,$\Delta H = (+)$ $2$. $\Delta S = (+)$
$c$. Reversible expansion of an ideal gas $3$. $\Delta S = (-)$

Which functions are required to understand the second law of thermodynamics?

Entropy is a measure of .......

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