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

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.

Text Solution

Verified by Experts

Non- spontaneous
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 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 ?

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

What is entropy change for the conversion of one gram of ice to water at 273 K and one atmospheric pressure? (DeltaH_("fusion")=6.025kJ" "mol^(-1))

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

The value of DeltaH and DeltaS for a reaction are respectively 30 kJ mol^(-1) and 100JK^(-1)mol^(-1) . Then temperature above which the reaction will become spontaneous is: