Question

Indicate whether you would expect the entropy of the system to increase or decrease in the following processes. Give reasons for your answer : (i) H2O (l, 373 K)®H2O (g, 373 K)

Answer 1

Answer:

See below.

Explanation:

The following process is given to us,

$H_{2}O_{\left( l\right) }\rightarrow H_{2}O_{\left( g\right)} \ at \ 373 \ K$

This process represents the change in the state of water, from liquid to gas ( vapour phase ).  

We know that the intermolecular forces of attraction are stronger in liquids than gases. In gases, the intermolecular distance being greater, these forces are not effective in bringing the molecules together.

In the gaseous state, the molecules are in continuous random motion and hence the entropy ( a measure of disorderedness ) is more than in liquids.

For processes in chemical equilibrium, we can write,

$\Delta S = \frac{\Delta H}{T}$

As we know that for boiling ( the process given to us ),

$\Delta H > 0 \\ \implies \Delta S > 0$

Heat is absorbed to change the state from liquid to solid.

Hence, the entropy increases in the given process.

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