The entropy change in the conversion of ...

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.

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At this temperature, water and ice will be at equilibrium

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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 ?

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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) .

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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))

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.

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