Chemical Reaction Rates Quiz

What is necessary for a chemical reaction to occur according to collision theory?

• Reactant particles must collide with sufficient energy and proper orientation.

• Reactant particles must be in a liquid state.

• Reactant particles must be heated to a high temperature.

• Reactant particles must be in a gaseous state.

How does an increase in the number of collisions affect the rate of a chemical reaction?

• It stops the reaction completely.

• It increases the rate of reaction.

• It has no effect on the rate of reaction.

• It decreases the rate of reaction.

Which equation is used to express the rate of reaction in terms of temperature?

• Boyle's Law

• Arrhenius Equation

• Ideal Gas Law

• Newton's Law

What is the relationship between concentration and the rate of reaction?

• They are unrelated.

• They are directly proportional.

• Concentration has no effect on the rate.

• They are inversely proportional.

What happens to the rate of reaction when the concentration of reactants is decreased?

• The rate decreases.

• The rate increases.

• The rate remains the same.

• The reaction stops.

How does increasing the surface area of a solid reactant affect the reaction rate?

• It stops the reaction.

• It has no effect on the reaction rate.

• It decreases the reaction rate.

• It increases the reaction rate.

What happens to the rate of reaction when the temperature is increased?

• The rate decreases.

• The rate remains the same.

• The reaction stops.

• The rate increases.

What role does a catalyst play in a chemical reaction?

• It decreases the activation energy required.

• It consumes the reactants.

• It has no effect on the reaction.

• It increases the activation energy required.

Which of the following is NOT a factor affecting the rate of chemical reactions?

• Concentration

• Surface area

• Color of reactants

• Temperature

What is the effect of a catalyst on the rate constant (k) in a reaction?

• It increases k.

• It has no effect on k.

• It makes k zero.

• It decreases k.