Home
Class 12
CHEMISTRY
The entropy change in the conversion of ...

The entropy change in the conversion of water to ice at 272 K for the system is -21.85 `JK^(-1) mol^(-1)` and that of surrounding is +21.93 `JK^(-1)mol^(-1)`. State whether the process is spontaneous or not ?

Text Solution

Verified by Experts

`Delta S_(total) = Delta S_(sys) + Delta S_(surr)`
`= - 21.85 JK^(-1) mol^(-1/0 + (+21.93 JK^(-1) mol^(-1))`
`= -0.08 JK^(-1) mol^(-1)`
`because` `Delta S_(process) lt 0 at 272 K`, the freezing of ice
`H_(2)O(I) rightarrow H_(2)O(s)` is a spontaneous process at 272 K.
Promotional Banner

Similar Questions

Explore conceptually related problems

The entropy change in the conversion of water to ice at 273 K for the system is -21.99 JK^(-1) mol^(-1) and that of surrounding is +21.99 JK^(-1)mol^(-1) . State whether the process is spontaneous or non-spontaneous.

The entropy change in the conversion of water to ice at 274 K for the system is -22.13 JK^(-1)mol^(-1) and for surrounding is +22.05 JK^(-1)mol^(-1) . State whether the process is spontaneous or non-spontaneous.

Find the entropy change for vaporisation of water to steam at 100^@C in JK^(-1)mol^(-1) if heat of vaporisation is 40.8 kJ mol^(-1) .

DeltaS_("surroundings")=+959.1 JK^(-1) mol^(-1) DeltaS_("system")=-163.1 JK^(-1) mol^(-1) Then the process is

A process has DeltaH=200Jmol^(-1) and DeltaS=40JK^(-1)mol^(-1) . The minimum temperature above which the process will be spontaneous is ___________K.

The entropy change for vaporisation of a liquid is 109.3JK^(-1)mol^(-1) . The molar heat of vaporisation of that liquid is 40.77 kJ mol^(-1) . Calculate the boiling point of that liquid.

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are -382.64 kJ mol^(-1) and -145.6 jK^(-1)mol^(-1) respectively. Standard Gibbs energy change for the same reaction at 298 K is

The entropy change for eaction at 300 K is 120 Jk^(-1) mol^(-1) . What is the enthalpy change for the reaction ?