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For some reaction carried out at constant atmospheric pressure and at a constant temperature of 25◦C, it is found that ∆H = −38.468 kJ/mol and ∆S = +51.4 J mol · K . What is the value of ∆G for this reaction under these conditions?

Respuesta :

sholadaniel1

Answer: ΔG =23.169kJ/mol

Explanation:

Solution

To Calculate Gibbs free energy ΔG for the reaction above we use the equation ΔG=ΔH−TΔS.

Where

ΔH= 38.468 kJ/mol = 38468 J/mol

∆S = +51.4 J mol−1 K−1).

T = 25◦C =298k

ΔG= 38468J/mol−298k(51.4 J mol−1 K−1).

ΔG = 38468 J/mol - 15317.2J/mol

ΔG = 23168.8J/mol

ΔG =23.169kJ/mol

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