Reaction Rates

Front

What is the definition of reaction rate?

Back

The reaction rate is the speed at which reactants are converted into products in a chemical reaction, typically measured in terms of concentration change over time.

Front

How does surface area affect reaction rates?

Back

Increasing the surface area of a reactant increases the reaction rate because it allows more particles to collide and react.

Front

What is activation energy (Ea)?

Back

Activation energy is the minimum energy required for a chemical reaction to occur.

Front

How does temperature affect reaction rates?

Back

Increasing the temperature generally increases the reaction rate because particles have more kinetic energy and collide more frequently and with greater energy.

Front

What is the effect of concentration on reaction rates?

Back

Increasing the concentration of reactants typically increases the reaction rate because there are more particles available to collide.

Front

What happens to the reaction rate when pressure is increased in gaseous reactions?

Back

Increasing pressure in gaseous reactions causes the reacting particles to move closer together, which increases the frequency of collisions and thus the reaction rate.

Front

What is a catalyst?

Back

A catalyst is a substance that increases the reaction rate without being consumed in the reaction by lowering the activation energy.

Front

What is the difference between a homogeneous and heterogeneous catalyst?

Back

A homogeneous catalyst is in the same phase as the reactants, while a heterogeneous catalyst is in a different phase.

Front

What is the rate law?

Back

The rate law is an equation that relates the rate of a reaction to the concentration of the reactants, often expressed as rate = k[A]^m[B]^n.

Front

What does the rate constant (k) represent in a rate law?

Back

The rate constant (k) is a proportionality constant that is specific to a particular reaction at a given temperature.