Collision Theory & Reaction Rates│Please Help!

Question

When solid sodium bicarbonate reacts with aqueous hydrogen monochlroride (hydrochloric acid) it forms carbon dioxide gas, water, and sodium chloride.

Which of the following would increase the rate of this reaction?

1. Increasing the pressure of the system
2. Heating the hydrochloric acid
3. Using larger crystals of sodium bicarbonate
4. Stirring the reactants
5. Using a higher concentration of hydrochloric acid

Answer 1

When solid sodium bicarbonate reacts with aqueous hydrogen monochlroride (hydrochloric acid) it forms carbon dioxide gas, water, and sodium chloride.

Which of the following would increase the rate of this reaction?

1. Increasing the pressure of the system

No. Since CO2 is produced, increasing pressure on the reaction will shift the equilibrium back toward the reactants by Le Chatelier's Law.

1. Heating the hydrochloric acid

Yes. Adding energy to the system will promote reaction.

1. Using larger crystals of sodium bicarbonate

No. Smaller crystals dissolve more readily to enhance reaction. Smaller crystals have more surface area per given mass.

1. Stirring the reactants

Yes. Stirring will enhance dissolution of the crystals so that the ions can react.

1. Using a higher concentration of hydrochloric acid

Yes. A higher hcl concentration on the reactants side will shift the equilibrium toward products (Le Chatelier's Law)