Midterm Question 6B
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Midterm Question 6B
Can anyone fully explain why question 6B on the midterm has answer A? I guessed that it is A because it is this reaction has the smallest change in entropy but I am not sure if that is correct.
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Re: Midterm Question 6B
Your logic is correct. Using the equation delta G = delta H - (T)(delta S), it is apparent that the value of delta G will be close to that of delta H when you have a value of delta S close to or equal to 0. Therefore, the answer with the smallest change in entropy, as you mentioned, would be the correct answer to this question.
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Re: Midterm Question 6B
Hiba Alnajjar_2C wrote:Your logic is correct. Using the equation delta G = delta H - (T)(delta S), it is apparent that the value of delta G will be close to that of delta H when you have a value of delta S close to or equal to 0. Therefore, the answer with the smallest change in entropy, as you mentioned, would be the correct answer to this question.
Why is answer b incorrect? (the reaction of sodium with water to make sodium hydroxide and H2 gas) I thought it would be spontaneous and exothermic (thus both g and h being negative)
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Re: Midterm Question 6B
Joseph Saba wrote:Hiba Alnajjar_2C wrote:Your logic is correct. Using the equation delta G = delta H - (T)(delta S), it is apparent that the value of delta G will be close to that of delta H when you have a value of delta S close to or equal to 0. Therefore, the answer with the smallest change in entropy, as you mentioned, would be the correct answer to this question.
Why is answer b incorrect? (the reaction of sodium with water to make sodium hydroxide and H2 gas) I thought it would be spontaneous and exothermic (thus both g and h being negative)
In answer b, you're going from a solid reactant and a liquid reactant to an aqueous product and a gas product. In answer a, you're going from solid reactants to solid products. Because the phase of the reactants is equivalent to that of the products in a, there is a very small change in entropy. This change would be smaller than that in b since the phases of the reactants and products in b are different; the overall entropy would increase in b whereas it wouldn't change very much in a. delta G and delta H being negative would not be enough for it to be considered as similar as they would be in answer a since the value of the term "-(T)(delta S)" would cause the values of delta G and delta H to be different in b since delta S is not zero.
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