Question

4. Given that the enthalpy of reaction for a system at 298 K is -292 kJ/mol and the entropy for that system is 224 J/mol K, what's the free energy for the system?

A.-87,793 kJ
B.-358 kJ
C.-225 kJ
D. -66,751 kJ​

Answer 1

B- 358 kj

Explanation: I took the test

Answer 2

`\Delta G=-359(kJ)/(mol)`

Step-by-step explanation:

Hello,

In this case, we must remember that the Gibbs free energy is defined in terms of the enthalpy, temperature and entropy as shown below:

`\Delta G=\Delta H -T\Delta S\\`

In such a way, for the given data, we obtain it, considering the conversion from J to kJ for the entropy in order to conserve the proper units:

`\Delta G=-292(kJ)/(mol) -(298)(224(J)/(mol)*(1kJ)/(1000J) )\\\\\Delta G=-359(kJ)/(mol)`

Best regards.