Concentration Changes Over Time AP Chemistry

AP Chemical Kinetics Review

By Andrew Baldwin

Multiple Choice

What is the rate of reaction?

• How fast a reaction is 
• How big a reaction is
• How loud a reaction is
• How much gas a reaction produces

Multiple Choice

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

Multiple Choice

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.

Multiple Choice

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

Multiple Choice

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

Multiple Choice

When surface area is decreased the rate of reaction...

• Decreases, because there are LESS possible sites for correct collisions

• Increases, because there are LESS possible sites for correct collisions

• Decreases, because there are MORE possible sites for correct collisions

• Increases, because there are MORE possible sites for correct collisions

Multiple Choice

How does a catalyst work in speeding up a reaction?

• By lowering the activation energy or reaction

• by giving them more energy

• by making them more available

Multiple Choice

The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?

• Red, because the activation energy is larger
• Blue, because the activation energy is lower
• both reaction progress at the same rate

Multiple Choice

You add more bodies into a "mosh pit" to hope for more collisions.  You have increased-

• temperature
• concentration
• pressure
• catalyst

Multiple Choice

• A. is most exothermic
• B. is most exothermic
• C. is most exothermic
• D. is most exothermic

Multiple Choice

Consider the following rate law: Rate = k[A]ⁿ[B]^m
How are the exponents n and m determined?

• by using balanced chemical equation
• By using the subscripts for the formulas
• By educated guess
• By experiment 

Multiple Choice

For 2A + B → 2C, the rate of production of C has been found to be 12 M/s. During that reaction, the rate of reaction was?

• 12 M/s
• 24 M/s
• 6 M/s
• Cannot tell without more data

Multiple Choice

The reaction of (CH₃)₃CBr with hydroxide ion proceeds:
(CH₃)₃CBr(aq) + OH^-(aq) → (CH₃)₃COH(aq) + Br^-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?

• 0.003
• 0.006
• 0.009
• 0.018

Multiple Choice

• rate = k[CO]²[O₂]²
• rate = k[CO]²[O₂]
• rate = k[CO][O₂]²
• rate = k[CO][O₂]^1/2

Multiple Choice

If you quadruple the concentration and the rate quadruples, what order is this reaction?

• zero

• first

• second

Multiple Choice

The particles under the purple curve (middle) have an average Kinetic Energy that is proportional to of 500K

• True

• False

Multiple Choice

___________ are produced in one step and used up in a later step and __________________ are present and unchanged in the reactants and the products

• intermediates, catalysts

• catalysts, intermediates

Multiple Choice

If a “reaction profile” has a taller ‘hill’ (or activation energy) then the reaction is ____________________?

• Faster

• Slower