Answer: The value of [tex]\Delta G[/tex] is -602.96 kJ/mol at 292 k for a reaction in which [tex]\Delta H[/tex] = 92 kj/mol and [tex]\Delta S[/tex] = 2.38 kj/mol K.
Explanation:
Given: Temperature = 292 K
[tex]\Delta H[/tex] = 92 kJ/mol
[tex]\Delta S[/tex] = 2.38 kJ/mol
Formula used to calculate the value of [tex]\Delta G[/tex] is as follows.
[tex]\Delta G = \Delta H - T\Delta S[/tex]
Substitute the values into above formula as follows.
[tex]\Delta G = \Delta H - T\Delta S\\= 92 kJ/mol - (292 K \times 2.38 kJ/mol K)\\= 92 kJ/mol - 694.96 kJ/mol\\= - 602.96 kJ/mol[/tex]
Thus, we can conclude that the value of [tex]\Delta G[/tex] is -602.96 kJ/mol at 292 k for a reaction in which [tex]\Delta H[/tex] = 92 kj/mol and [tex]\Delta S[/tex] = 2.38 kj/mol K.
