Journal Entry:

Some over-the-counter antacids contain mineral carbonates (CaCO₃), MgCO₃) as their primary ingredient. A chemistry student want to optimize the efficacy of the antacid to neutralize stomach acid (HCl). Which of the following would be expected to increase the rate at which the mineral carbonates neutralize HCl in vitro (not in the biological system)?

(A) increase volume of the reaction solution
(B) Increase pressure on the solution
(C) Decrease particle size of the tablets by grinding them into a powder.
(D) Decrease the temperature at which the reaction occurs.

Learning Intentions

• We will learn how reaction rate is calculated.

• We will learn how to interpret results of experiments regarding factors that may  influence the rate of a reaction. 

• We will learn how to draw energy profile, particulate and/or symbolic representation of a chemical reaction occurring in difference situations to show effect of conditions.

• We will learn how to analyze concentration vs time data to determine the rate law for zeroth, first and second order reaction. 

Closing Task:

You can analyze concentration vs time data to determine rate law equations for a chemical reaction.

Content Standards being covered:

The rate of a reaction is influenced by the concentration or pressure of reactants, the phase of the reactants and products, and environmental factors such as temperature and solvent. (E.K. 4.A.1)

Catalysts function by lowering the activation energy of an elementary step in a reaction mechanism, and by providing a new and faster reaction mechanism. (E.K. 4.D.1)

The rate law shows how the rate depends on reactants concentrations. (E.K. 4.A.2)