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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.

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To determine whether the conversion of water to ice at 274 K is spontaneous or non-spontaneous, we need to analyze the changes in entropy for both the system and the surroundings. ### Step-by-Step Solution: 1. **Identify the given values**: - Change in entropy for the system (ΔS_system) = -22.13 J/K·mol - Change in entropy for the surroundings (ΔS_surroundings) = +22.05 J/K·mol ...
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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 ?

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 ?

The entropy change for vapourisation of liquid water to steam 100^@C is …. JK^(-1) mol^(-1) . Given that heat of vapourisation is 40.8 kJ mol^(-1) .

The units of DeltaS are JK^(-1) mol^(-1) .

Dependence of Spontaneity on Temperature: For a process to be spontaneous , at constant temperature and pressure , there must be decrease in free energy of the system in the direction of the process , i.e. DeltaG_(P.T) lt 0. DeltaG_(P.T) =0 implies the equilibrium condition and DeltaG_(P.T) gt 0 corresponds to non- spontaneity. Gibbs- Helmholtz equation relates the free energy change to the enthalpy and entropy changes of the process as : " "DeltaG_(P.T) = DeltaH-TDeltaS" ""..."(1) The magnitude of DeltaH does not change much with the change in temperature but the entropy factor TDeltaS change appreciably . Thus, spontaneity of a process depends very much on temperature. For endothermic process, both DeltaH and DeltaS are positive . The energy factor, the first factor of equation, opposes the spontaneity whereas entorpy factor favours it. At low temperature the favourable factor TDeltaS will be small and may be less than DeltaH, DeltaG will have positive value indicated the nonspontaneity of the process. On raising temperature , the factor TDeltaS Increases appreciably and when it exceeds DeltaH, DeltaG would become negative and the process would be spontaneous . For an expthermic process, both DeltaH and DeltaS would be negative . In this case the first factor of eq.1 favours the spontaneity whereas the second factor opposes it. At high temperature , when T DeltaS gt DeltaH, DeltaG will have positive value, showing thereby the non-spontaneity fo the process . However , on decreasing temperature , the factor , TDeltaS decreases rapidly and when TDeltaS lt DeltaH, DeltaG becomes negative and the process occurs spontaneously. Thus , an exothermic process may be spontaneous at low temperature and non-spontaneous at high temperature. The enthalpy change for a certain rection at 300 K is -15.0 K cal mol^(-1) . The entropy change under these conditions is -7.2 cal K^(-1)mol^(-1) . The free energy change for the reaction and its spontaneous/ non-spontaneous character will be

Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (DeltaG)_(PT) = DeltaH - T DeltaS The magnitude of DeltaH does not change much with the change in temperature but the enrgy factor T DeltaS changes appreciably. Thus, spontaneity of a process depends very much on temperature. The enthalpy change for a certain reaction at 300K is -15.0 kcal mol^(-1) . The entropy change under these conditions is -7.2 cal K^(-) mol^(-1) . The free enegry change for the reaction and its spontaneous//nonspontaneous character will be

At 373 K, the entropy change for the transition of liquid water to steam (DeltaS_("vap")) is 109 J K^(-1) mol^(-1) . Calculate the enthalpy change (Delta_("vap")H) for the process.

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

If the entropy of vaporisation of a liquid is 110 JK^(-1)mol^(-1) and its enthalpy of vaporisation is 50 kJ mol^(-1) . The boiling point of the liquid is

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