# Problem: The standard molar Gibbs free energy of formation of NO 2 (g) at 298 K is 51.30 kJ·mol−1 and that of N2O4 (g) is 97.82 kJ·mol−1. What is the equilibrium constant at 25°C for the reaction2 NO2(g) ⇌ N2O4(g) ?1. 6.882. 0.1453. 7.01 × 10−94. 1.005. None of these6. 1.02 × 10−107. 9.72 × 1098. 0.657

###### FREE Expert Solution
94% (283 ratings)
###### Problem Details

The standard molar Gibbs free energy of formation of NO 2 (g) at 298 K is 51.30 kJ·mol−1 and that of N2O4 (g) is 97.82 kJ·mol−1. What is the equilibrium constant at 25°C for the reaction
2 NO2(g) ⇌ N2O4(g) ?

1. 6.88

2. 0.145

3. 7.01 × 10−9

4. 1.00

5. None of these

6. 1.02 × 10−10

7. 9.72 × 109

8. 0.657

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofThe standard molar Gibbs free energy of formation of NO 2 (g...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 9 minutes and 25 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Bruehl's class at CU.