At what temperature will the following reaction happen spontaneously, given that ΔH=8.91×103J and ΔS= –219.20 J/K? CaSO4(s) + 2HCl(g) → CaCl2(s) + H2SO4(l)A) at 298 K
B) at 100 K
C) It is spontaneous at any temperature.
D) It is not spontaneous at any temperature.
Answers
Answer:
D) It is not spontaneous at any temperature.
Explanation:
Given reaction:
CaSO4(s) + 2HCl(g) → CaCl2(s) + H2SO4(l)
ΔH = +8.91*10³ J
ΔS = -219.20 J/K
The sign of the Gibbs free energy (ΔG) determines the spontaneity of a given reaction. ΔG is related to ΔH and ΔS as follows:
A reaction is spontaneous only when ΔG is negative i.e. ΔG < 0
Under the given conditions:
ΔH > 0 ; ΔS <0 and ΔH > ΔS
i.e. ΔG = ('+' value) - T( '- 'value) = + value
Therefore, irrespective of the temperature, ΔG will always be positive
For this reaction DH>0 and DS<0. So, d. the reaction is not spontaneous at any temperature.
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What is pOH?
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The type of food and therefore the amount of food that is a gift in your epithelial duct once you consume alcohol have the foremost direct impact on the speed of alcohol absorption.
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