Question

What is the value of the equilibrium constant, K, for a reaction for which ∆G° is equal to –5.20 kJ at 50°C?

Answer 1

Answer:

6.93

Explanation:

Step 1: Given data

• Standard Gibbs free energy (∆G°): -5.20 kJ

• Temperature (T): 50°C

• Equilibrium constant (K): ?

Step 2: Convert the temperature to the Kelvin scale

We will use the following expression.

K = °C + 273.15

K = 50°C + 273.15

K = 323 K

Step 3: Calculate K

We will use the following expression.

∆G° = -R × T × ln K

-5.20 × 10³ J = -(8.314 J/mol.K) × 323 K × ln K

K = 6.93