At what temperature will the following reaction happen spontaneously, given that ΔH = 8.91*103 J/mol and ΔS = - 219.20 J/mol·K? CaSO4 (s) + 2HCl (g) → CaCl2 (s) + H2SO4 (l)

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Rolex

Chemistry

4 September, 02:08

At what temperature will the following reaction happen spontaneously, given that ΔH = 8.91*103 J/mol and ΔS = - 219.20 J/mol·K? CaSO4 (s) + 2HCl (g) → CaCl2 (s) + H2SO4 (l)

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Nyla Chang · Answer 1

In order for a certain reaction to be spontaneous, the change in Gibb's free energy must be negative, that is:

dG < 0

We can calculate dG using:

dG = dH - dS

When we plug in the given values, we see that the sign of dG will never be negative; therefore, the reaction will not be spontaneous under any conditions.