Unit 11: Kinetics Final Exam Review

Which of the following increase the reaction rate?

• less surface area

• lower temperature

• increasing pressure

• increased concentration

A catalyst works by

• changing the order of the reaction
• increasing the temperature
• lowering the activation energy
• making the activated complex

If the temperature is reduced, a reaction rate will ______

• increase

• decrease

• stay the same

Use the graphs to answer the following question. 

Which reaction would be the MOST difficult reaction to accomplish  and why?

• Reaction 1, because it takes less energy for the reactants to reach the transition state.

• Reaction 2, because it takes less energy for the reactants to reach the  transition state.

• Reaction 1, because it takes more energy for the reactants to reach the  transition state.

• Reaction 2, because it takes more energy for the reactants to reach the  transition state. 

Use the information and graphs to answer the following question. Both graphs represent the same reaction. Which of the following correctly identifies the reaction that was  carried out with a catalyst? 

• Trial 1, because it decreased the rate of the reaction. 

• Trial 2, because it decreased the rate of the reaction.

•  Trial 1, because it decreased the activation energy needed for the  reaction to occur. 

• Trial 2, because it decreased the activation energy needed for the  reaction to occur.

In a lab, students are given 100.0 mL of 1M hydrochloric acid, HCl, to  make a product. Which of the following steps should the students  take in order to increase the rate of reaction between hydrochloric  acid and sugar?  

• Increase the concentration of hydrochloric acid to 2M because greater  concentrations result in more collisions between the reactants.

•  Increase the volume of hydrochloric acid to 200.0 mL because a greater  amount of reactant results in a faster reaction rate.  

• Decrease the concentration of hydrochloric acid to 0.5M because lower  concentrations result in more collisions between the reactants.

• Decrease the volume of hydrochloric acid to 50.0 mL because a lower  amount of reactant results in a faster reaction rate. 

Use the information to answer the following question. 

Several groups of Chemistry students are tasked with producing aluminum  chloride using solid aluminum as a reactant. The teacher provides the  students with two forms of aluminum, powder and solid chunks.  

Which type of aluminum should the students plan to use in order to  increase the reaction rate? 

•  Powder because the lower surface area will allow more collisions  between reactants to occur.

•  Powder because the greater surface area will allow more collisions  between reactants to occur.

• Solid chunks because the lower surface area will allow more collisions  between reactants to occur.

• Solid chunks because the greater surface area will allow more collisions  between reactants to occur. 

What criteria must be met for reactant collisions to result in a successful product?

• The reactants must collide with each other

• The reactants must collide with enough energy and be in the right positions

• The reactants must have enough energy to form the activated complex

More collisions correspond to a: 

• Faster reaction rate  
• Slower reaction rate
• Constant reaction rate 
• None of the above

Increase in temperature of the reactants can do one of the following

• Slow collision frequency
• Allow less effective collision between the particles
• Neutralise the reaction
• increase collision between the particles thus increasing the rate.