Why don't all thermodynamically favored reactions occur rapidly?

a. Because thermodynamics and reaction rates are unrelated properties.

b. The reactants still need to break bonds and overcome the activation energy in order to form products.

c. The equilibrium of the reaction favors the reactants and not the products.

d. Because thermodynamically favored reactions have positive free energy.

Question

Cameron Barnes

Physics

31 December, 11:59

Why don't all thermodynamically favored reactions occur rapidly?

a. Because thermodynamics and reaction rates are unrelated properties.

b. The reactants still need to break bonds and overcome the activation energy in order to form products.

c. The equilibrium of the reaction favors the reactants and not the products.

d. Because thermodynamically favored reactions have positive free energy.

+3

Answers (1)

Know the Answer?

Blaze Garner · Answer 1

b

Explanation:

A thermodynamic-ally favored reactions are nothing but spontaneous reactions. In spontaneous reactions ΔH (enthalpy) is always negative and ΔS (entropy) is always positive.

Now all thermodynamic-ally favored reactions does not occur rapidly because the reactants still need to break bonds and overcome the activation energy in order to form products.