Reaction Rates

Grinding an seltzer tablet into a powder increases the rate of reaction due to increased

• concentration.

• surface area.

• temperature.

• reactants.

Which factors increase the rate of a chemical reaction?

• increasing temperature

• increasing concentration

• increasing surface area

• all of these

A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 

• catalyst
• product
• reactant
• solute

Why does a higher temperature increase the rate of a reaction?

• it increases both the frequency and energy of particle collisions
• it only increases the frequency of particle collisions
• it only increases the energy of particle collisions
• it reduces the activation energy of the reaction

Why does a higher concentration increase the rate of reaction?

• it increases the amount of reactants
• it lowers the activation energy
• it increases the energy of particle collisions
• it increases the frequency of particle collisions because there are more collision sites

In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate the slowest? 

• A

• B

• C

• D

Which of the following would increase the number of collisions that occur?

(choose all that apply)

• increased surface area

• decreased concentration

• increased temperature

• increased volume

How could we make this reaction happen more quickly?

• decrease the concentration of the acid

• crush the chalk to increase the surface area

• put the test tube in an ice bath

• increase the amount of acid

AgNO₃ + NaCl → AgCl + NaNO₃

What would you expect to happen if we decrease the temperature of this reaction container?

• The energy of the reactants would decrease.

• There would be more product produced.

• The number of particles of

  AgNO₃ and NaCl would decrease.

• The number of collisions in the reactants would increase.

More collisions (in the correct orientation) results in

(choose all that apply)

• a slower reaction rate.

• an increased reaction rate.

• more product being produced.

• less volume of the reaction container.