Increasing temperature generally increases the rate of a chemical reaction.

In a first-order reaction, increasing the concentration of a reactant results in a linear increase in the rate.

Increasing the concentration of reactants generally increases the rate of a reaction.

Increasing the pressure increases the concentration of gaseous reactants, which generally increases the rate of reaction.

The integrated rate law for a first-order reaction is ln[A] = -kt + ln[A]0.

If the rate constant has the unit L/mol·s, the reaction is second order.

The rate law expression is derived directly from the rate equation, which is given as rate = k[A]^2[B].

The unit of the rate constant for a second-order reaction is L²/mol²·s.

The color of the reactants does not affect the rate of a chemical reaction.

A catalyst lowers the activation energy of a reaction, thereby increasing the rate.

In a first-order reaction, the rate is directly proportional to the concentration of the reactant.

The Arrhenius equation relates temperature to the rate constant and includes the activation energy.

The rate of reaction generally increases with increasing concentration of reactants.

Catalysts provide an alternative pathway with lower activation energy, thus increasing the rate of the reaction without being consumed.

In an endothermic reaction, the enthalpy change (ΔH) is positive as heat is absorbed.

A catalyst lowers the activation energy of a reaction, thereby increasing the rate without being consumed.

Catalysts provide an alternative pathway with a lower activation energy, thus increasing the reaction rate without being consumed.

The activation energy (Ea) of a reaction is always positive.

Activation energy is always positive as it represents the minimum energy required for a reaction to occur.

The rate of a reaction generally increases with increasing temperature.

The rate of reaction decreases with time for a reactant and increases with time for a product.