<u>Answer:</u>
<u>For 1:</u> The enthalpy change for the given reaction is -176000 J.
<u>For 2:</u> Yes, the negative sign of the gibbs free energy represents a spontaneous reaction.
<u>Explanation:</u>
For the given chemical reaction:
We are given:
= Gibbs free energy = -91368 J
T = Temperature =
= entropy of the reaction = -284 J/K
To calculate the enthalpy of the reaction, we use the equation for gibbs free energy, which is:
Putting values in above equation, we get:
Hence, the enthalpy change for the given reaction is -176000 J.
Gibbs free energy is defined as the energy which is available to do some work. It is represented as
Sign convention for
- If value comes out to be positive, it is considered as non-spontaneous reaction.
- If value comes out to be negative, it is considered as spontaneous reaction.
So, yes the negative sign of the gibbs free energy represents a spontaneous reaction.