The unit of rate constant for a first-order reaction is:

The half-life of a first-order reaction is:

Activation energy is the:

Arrhenius equation is: k =

A catalyst increases reaction rate by:

For a zero-order reaction, the rate is:

Molecularity of an elementary reaction is:

The rate law can be determined from:

Temperature coefficient of a reaction is usually:

In a pseudo-first-order reaction:

The integrated rate equation for first order is:

Collision theory requires effective collisions to have:

The order of a reaction is determined by:

Half-life of a zero-order reaction is:

Enzyme catalysis follows:

For a second-order reaction, the plot of 1/[A] vs t is:

Rate of reaction at equilibrium is:

The slowest step in a reaction mechanism is called:

A reaction has Ea = 0. This means:

Photochemical reactions are initiated by: