Which of these is spontaneous at low temperatures?*A system with ΔHᵒ>0; ΔSᵒ<0A system with ΔHᵒ<0; ΔSᵒ<0A system with ΔHᵒ<0; ΔSᵒ>0A system with ΔHᵒ>0; ΔSᵒ>0
Question
Which of these is spontaneous at low temperatures?*A system with ΔHᵒ>0; ΔSᵒ<0A system with ΔHᵒ<0; ΔSᵒ<0A system with ΔHᵒ<0; ΔSᵒ>0A system with ΔHᵒ>0; ΔSᵒ>0
Solution
The spontaneity of a reaction can be determined using the Gibbs Free Energy equation: ΔG = ΔH - TΔS.
A reaction is spontaneous if ΔG < 0.
Let's analyze each option:
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A system with ΔHᵒ>0; ΔSᵒ<0: In this case, ΔG = ΔH - TΔS will be positive because both terms are positive (ΔH is positive and -TΔS is also positive because ΔS is negative). So, this reaction is not spontaneous at any temperature.
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A system with ΔHᵒ<0; ΔSᵒ<0: In this case, ΔG = ΔH - TΔS will be negative at low temperatures because ΔH is negative and -TΔS is less negative (because ΔS is negative and T is low). So, this reaction is spontaneous at low temperatures.
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A system with ΔHᵒ<0; ΔSᵒ>0: In this case, ΔG = ΔH - TΔS will always be negative because both terms are negative (ΔH is negative and -TΔS is also negative because ΔS is positive). So, this reaction is spontaneous at all temperatures.
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A system with ΔHᵒ>0; ΔSᵒ>0: In this case, ΔG = ΔH - TΔS will be negative at high temperatures because ΔH is positive and -TΔS is negative but becomes more negative as T increases (because ΔS is positive). So, this reaction is spontaneous at high temperatures.
So, the answer is: A system with ΔHᵒ<0; ΔSᵒ<0 is spontaneous at low temperatures.
Similar Questions
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Which statement is true regarding a process for which ΔH is positive and ΔS is negative? Recall that, for any process: ΔG = ΔH - TΔSSelect answer from the options belowThe process is spontaneous at low temperatures only.The process is not spontaneous at any temperature.The process is spontaneous at all temperatures.The process is spontaneous at high temperatures only.
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