For a particular reaction, ΔH = 139.99 kJ/mol and ΔS = 298.7 J/(mol·K). Calculate ΔG for this reaction at 298 K.
?=____kJ/mol
What can be said about the spontaneity of the reaction at 298 K?
A. The system is spontaneous as written.
B.The system is at equilibrium.
C. The system is spontaneous in the reverse direction.

Answers

Answer 1

The ΔG for this reaction at 298 K is 50.98 kJ/mol. In terms of the spontaneity of the reaction at 298 K, it can be said that C. The system is spontaneous in the reverse direction.

To calculate ΔG for the reaction at 298 K, use the equation for the Gibbs free energy:
ΔG = ΔH - TΔS

In this case,
ΔH = 139.99 kJ/mol
ΔS = 298.7 J/(mol·K)
Temperature (T) = 298 K

First, convert ΔS to kJ/(mol·K) by dividing by 1000:
ΔS = 298.7 J/(mol·K) ÷ 1000 = 0.2987 kJ/(mol·K)

Now, plug in the values into the equation:
ΔG = 139.99 kJ/mol - (298 K × 0.2987 kJ/(mol·K))

ΔG = 139.99 kJ/mol - 89.01 kJ/mol
ΔG = 50.98 kJ/mol

Since ΔG > 0, the reaction is not spontaneous in the forward direction at 298 K. Therefore, the correct answer is:

C. The system is spontaneous in the reverse direction.

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