AP Kinetics Review Game

Which of the following will most likely increase the rate of the reaction represented above?

• Decreasing the temperature of the reaction system

• Adding a heterogeneous catalyst to the reaction system

• Increasing the volume of the reaction vessel using a piston

• Removing some H₂ (g) from the reaction system

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NGSS.HS-PS1-5

• I only

• II only

• I and II only

• I, II, and III

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NGSS.HS-PS1-4

What effect will increasing [H⁺] at constant temperature have on the reaction represented?

• The activation energy of the reaction will increase.

• The activation energy of the reaction will decrease.

• The frequency of collisions between H⁺ and ClO^- will increase.

• The value of the rate constant will increase.

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NGSS.HS-PS1-5

Two sample of Mg of equal mass were placed in equal of HCl contained in two separate reaction containers. Particle diagrams of the mixing of Mg and HCl in the reaction containers are shown in Figures 1 and 2. Which of the reactions will proceed faster, and why?

• The reaction in Figure 1, because the atoms of Mg are more concentrated than those in Figure 2.

• The reaction in Figure 1, because the Mg in Figure 1 has a larger mass than the Mg in Figure 2.

• The reaction in Figure 2, because more Mg atoms are exposed to HCl in Figure 2 than Figure 1.

• The reaction in Figure 2, because the Mg in Figure 2 has less surface area than the Mg in Figure 1.

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NGSS.HS-PS1-5

Two solid reactions of varying particle size are combined in a vessel. Assuming that the same mass of each reactant is used in each case, which of the following represents the conditions that will result in the fastest reaction rate?

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NGSS.HS-PS1-5

Which of the following best helps explain why an increase in temperature increases the rate of a chemical reaction?

• At higher temperatures, reactions have a lower activation energy.

• At higher temperatures, reactions have a higher activation energy.

• At higher temperatures, every collision results in the formation of a product.

• At higher temperatures, high-energy collisions happen more frequently.

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NGSS.HS-PS1-5

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NGSS.HS-PS1-5

• Rate = k[NO][O₂]

• Rate = k[NO][O₂]²

• Rate = k[NO]²[O₂]

• Rate = k[NO]²[O₂]²

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NGSS.HS-PS1-5

After a certain pesticide compound is applied to crops, its decomposition is a first-order reaction with a half-life of 32.5 days. What is the rate constant, k, for the decomposition reaction?

• 0.0213 day^-1

• 0.0308 day^-1

• 32.5 day^-1

• 46.9 day^-1

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NGSS.HS-PS1-5