Chapter 5 Test

Question 1

Practice writing rate law with experimental data

Answer 1

• 5.2 problems

Question 2

At what point in time during a chemical reaction should the reaction have the greatest value?

Answer 2

At the very beginning when time= zero. The initial rate is the fastest rate because the concentration of the reactants is at its highest value and a higher concentration of reactants results in more effective collisions and a higher rate

Question 3

Practice 5.9 with the substitution problems

Question 4

Review video problems on classroom with that one teacher

Answer 4

5.1- # 3
5.3- #16, 17
5.5- #6

Question 5

If you have a small rate constant, what is the relative speed of the reaction typically? And if you have a large rate constant?

Answer 5

Slow; Fast

Question 6

Practice problems on khan academy

Question 7

When you increase the temperature how does it affect k?

Answer 7

K goes up and the opposite for if you decrease it

Question 8

How do you create a rate law for an equation with the slow step as the second step?

Answer 8

Create your rate law as normal, but if there are intermediates included in your rate then you have to do substitution. If it is an easy/obvious substitution do that, but if not, then make sure your equation you are substituting is equilibrium, then do subtraction to make the equation equal to what you need to substitute, then put any negative reactants on the bottom to get your final rate law.

Question 9

Study the 5.4-5.8 quizlet

Question 10

Study 5.1-5.3 Quizlet

Question 11

Which of the following does not influence reaction rates? Be able to explain why as well.

• the rate of collisions between reactant molecules
• the activation energy
• the orientation of collisions between reactant molecules
• the difference of potential energy between reactants and products

Answer 11

• the difference of potential energy between reactants and products

Question 12

Describe TWO reasons why the pressure changes as the temperature of the C2H4(g) increases. Your descriptions must be in terms of what occurs at the molecular level.

Answer 12

• The pressure increases because the temperature increase causes more frequent collisions
• The pressure increases because the temperature increase causes collisions to be more powerful

Question 13

When HCl(g) is injected into the container of C2H4(g) at 450 K, the total pressure increases. Then, as the reaction proceeds at 450 K, the total pressure decreases. Explain this decrease in total pressure in terms of what occurs at the molecular level. There is a balanced equation available and the equation is exothermic.

Answer 13

The decrease in pressure after the initial increase is a consequence of the reaction that produces fewer gas molecules than it consumes. When fewer gas molecules are present, there are fewer collisions with the container walls, resulting in a decrease in pressure.

Question 14

The reaction is first order. Explain how the data in the table are consistent with a first-order reaction.

Answer 14

For a first-order reaction, the half-life is independent of reactant concentration (or pressure) at constant T, as shown in trials 1, 2, and 3.

Question 14

Practice 2014, 2015, 2016, 2022 frq

Question 14

Practice the photoelectron spectrum

Question 15

How do you writte a net ionic equation?

Answer 15

Include all charges and take out all spectator ions. Keep all solids, gases, and liquids together.