System Change ? S A few moles of nitrogen (N 2 ) gas. <? S 0 =? S 0 >? S 0 not e
ID: 863298 • Letter: S
Question
System
Change
?S
A few moles of nitrogen (N2) gas.
<?S0
=?S0
>?S0
not enough information
A few grams of liquid acetone ((CH3)2CO).
<?S0
=?S0
>?S0
not enough information
A few moles of nitrogen (N2) gas.
<?S0
=?S0
>?S0
not enough information
System
Change
?S
A few moles of nitrogen (N2) gas.
<?S0
=?S0
>?S0
not enough information
A few grams of liquid acetone ((CH3)2CO).
<?S0
=?S0
>?S0
not enough information
A few moles of nitrogen (N2) gas.
<?S0
=?S0
>?S0
not enough information
(having trouble with the last one. I'd still appreciate if you give your input on all three though)
For each system listed in first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy of the system, decrease , or leave unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.
Explanation / Answer
1.the process described is a reversible isothermal process.The reversible process has zero total change in entropy..here the process is reversible so entropy change is 0.hence option 2
2.In the question the work done is phase change .For phase change we all know the change in enrtopy is increased,since randomeness increases from solid to gas and entropy is a measure of randomeness(from 2 law of thermodynamics).So its option C i.e. S>0
3.Here once a gas is cooled at constant volume and it is expanded at constant temperature.So for the temperature change process S=0 since it is reversible .But for volume change process gas undergoes expansion so randomeness increases and S>0 .So overall there is an increase in entropy i.e.S>0.
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