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The signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all temperatures would be respectively
- a)(+, +, −)
- b)(+, −, +)
- c)(−, −, −)
- d)(+, +, +)
Correct answer is option 'B'. Can you explain this answer?
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The signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all tem...
Signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all temperatures would be (-, -, +). Let's break this down further:
ΔH: Enthalpy change
- A negative ΔH indicates an exothermic reaction, where heat is released.
- A positive ΔH indicates an endothermic reaction, where heat is absorbed.
- For a non-spontaneous reaction, the reactants have more energy than the products. Therefore, the ΔH will be positive.
ΔS: Entropy change
- A positive ΔS indicates an increase in randomness or disorder.
- A negative ΔS indicates a decrease in randomness or disorder.
- For a non-spontaneous reaction, the reactants are more ordered than the products. Therefore, the ΔS will be negative.
ΔG: Free energy change
- A negative ΔG indicates a spontaneous reaction, where the products are favored.
- A positive ΔG indicates a non-spontaneous reaction, where the reactants are favored.
- For a non-spontaneous reaction, both ΔH and ΔS are positive. Therefore, the ΔG will be positive as well.
Combining all of this information, we can see that the signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all temperatures would be (-, -, +), which corresponds to option B.
ΔH: Enthalpy change
- A negative ΔH indicates an exothermic reaction, where heat is released.
- A positive ΔH indicates an endothermic reaction, where heat is absorbed.
- For a non-spontaneous reaction, the reactants have more energy than the products. Therefore, the ΔH will be positive.
ΔS: Entropy change
- A positive ΔS indicates an increase in randomness or disorder.
- A negative ΔS indicates a decrease in randomness or disorder.
- For a non-spontaneous reaction, the reactants are more ordered than the products. Therefore, the ΔS will be negative.
ΔG: Free energy change
- A negative ΔG indicates a spontaneous reaction, where the products are favored.
- A positive ΔG indicates a non-spontaneous reaction, where the reactants are favored.
- For a non-spontaneous reaction, both ΔH and ΔS are positive. Therefore, the ΔG will be positive as well.
Combining all of this information, we can see that the signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all temperatures would be (-, -, +), which corresponds to option B.
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The signs of ΔH, ΔS, and ΔG for a non-spontaneous reaction at all tem...
ΔG=+vefor non-spontaneous reactions
As ΔG = ΔH − TΔS
Thus ΔH should be positive and ΔS should be negative, thus ΔG will be positive at all temperatures.
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