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.

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.

speed

ratio of distance traveled to time interval

net force

vector sum of forces on object

object

source of diverging light rays either luminous or illuminated

don't remove my answer im trying my best to answer them

explanation:

the body's situation won't change the forces are equal opposit and on the same body