Answer :
Answer:
The correct option is: ΔSsurr is greater than 0 and its magnitude is greater than ΔSsys.
Explanation:
For a chemical reaction to be spontaneous, the change in the Gibbs free energy should be negative (ΔG = -ve).
At constant temperature (T) and pressure, the Gibbs free energy is given by the equation: [tex]\Delta G_{system} = \Delta H_{system} - T\Delta S_{system}[/tex]
Here, [tex]\Delta H_{system}[/tex] is the enthalpy change and [tex]\Delta S_{system}[/tex] is the entropy change of the system.
Also, according to the second law of thermodynamics, for a spontaneous process, the total entropy, [tex]\Delta S_{universe} = \Delta S_{system} + \Delta S_{surrounding} > 0[/tex]
Therefore, for a reaction to be spontaneous, if [tex]\Delta S_{system}[/tex] is less than 0 or negative; then [tex]\Delta S_{surrounding}[/tex] should be greater than 0 or positive. Also, [tex]\Delta S_{surrounding}[/tex] > [tex]\Delta S_{system}[/tex].
Correct choice: ΔSsurr is greater than 0 and its magnitude is greater than ΔSsys.
Facts about Gibb's free energy:
- For a chemical reaction to be spontaneous, the change in the Gibbs free energy should be negative (ΔG = -ve).
- At constant temperature (T) and pressure, the Gibbs free energy is given by the equation: ΔG=ΔH-TΔS
- Here, ΔH is the enthalpy change and ΔS is the entropy change of the system.
- From, the second law of thermodynamics, we know that for a spontaneous process, the total entropy, [tex]\triangle S_{universe}=\triangle S_{system}+\triangle S_{surrounding}>0[/tex]
- Therefore, for a reaction to be spontaneous, if ΔSsys is less than 0 or negative; then ΔSsurr should be greater than 0 or positive. Also,[tex]\triangle S_{surrounding}>\triangle S_{system}[/tex] .
Thus, the correct option is given above.
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