Question

Consider the hypothetical chemical reactions:

a⇌b,Δr​G=12.30kJ mol⁻¹

b⇌c,Δr​G=−26.70kJ mol⁻¹

c⇌d,Δr​G=5.20kJ mol⁻¹

What is the Gibbs energy change, Δr​G, for the overall reaction a⇌d? Express your answer with the appropriate units.

Answer 1

The Gibbs energy change (ΔrG) for the overall reaction a ⇌ d is -9.20 kJ/mol.

Step-by-step explanation:

The Gibbs energy change (ΔrG) for the overall reaction a ⇌ d can be calculated by summing the individual ΔrG values of the reactions involved. The overall reaction can be represented as a combination of the three reactions given:

a ⇌ b (ΔrG = 12.30 kJ/mol)

b ⇌ c (ΔrG = -26.70 kJ/mol)

c ⇌ d (ΔrG = 5.20 kJ/mol)

By summing the ΔrG values, we get:

ΔrG (overall) = ΔrG (a ⇌ b) + ΔrG (b ⇌ c) + ΔrG (c ⇌ d)

= 12.30 kJ/mol + (-26.70 kJ/mol) + 5.20 kJ/mol

= -9.20 kJ/mol

Therefore, the Gibbs energy change (ΔrG) for the overall reaction a ⇌ d is -9.20 kJ/mol.