Question

Examine the following reaction.

N2 (g)+3H2 (g)⇋2NH3 (g)ΔH0ΔS0=−92.0 kJ=−0.198 J/K
What is the correct value for free energy of this reaction at 300 K?

Answer 1

Step-by-step explanation:

To calculate the free energy change (ΔG) of the reaction at 300 K, we can use the equation:

ΔG = ΔH - TΔS

where:

ΔH = Enthalpy change

ΔS = Entropy change

T = Temperature in Kelvin

Given:

ΔH = -92.0 kJ (convert to J by multiplying by 1000, so ΔH = -92,000 J)

ΔS = -0.198 J/K

T = 300 K

Now, substitute the values into the equation:

ΔG = -92,000 J - (300 K) * (-0.198 J/K)

ΔG = -92,000 J + 59.4 J

ΔG = -91,940.6 J

The correct value for the free energy change of the reaction at 300 K is approximately -91,940.6 Joules (J).