13.1 Rates of Reaction

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

Order the letters from highest to lowest rate of reaction.

• A > B > C > D

• A > BC > D (B and C have the same rate)

• A > B > CD (C and D have the same rate)

• D > C > B > A

Multiple Choice

The graph below shows how the concentrations of reactants and products change during a chemical reaction. Which line is likely to be the reactant?

• A, blue

• B, red

• C, green

Multiple Choice

Which size marble chips produced the quickest rate of reaction when added to HCl.

• Small

• Medium

• Large

• I dont know

Multiple Choice

Which temperature in Celsius provided the quickest reaction speed.

• 40

• 30

• 50

• 10

Multiple Choice

As time passes the reaction rate starts to...

• Speed up

• Stay the same

• Slow down

• Not change

Multiple Choice

What does a horizontal (flat line) on a reaction graph tell us?

• Reaction in slowing down

• Reaction is speeding up

• Reactant has been used up

Multiple Choice

Read the image

• 0.005

• 0.0025

• 0.00123

• 0.025

Multiple Choice

For the same reaction between hydrogen and iodine, suppose you have a product concentration of 0.180 mol/L at time t1 = 15 s and a concentration of 0.205 mol/L at time t2 = 20 s. Calculate the average reaction rate for the time interval with respect to the product, HI.

• 0.005

• 0.0025

• 0.00123

• 0.025

Multiple Choice

Table 4 shows the total volume of gas evolved at different intervals for the decomposition of hydrogen peroxide.

What is the average rate of reaction in from time=1.0min to time=2.0min?

• 14.0 cm³ min^-1

• 16.0 cm³ min^-1

• 18.0 cm³ min^-1

• 28.0 cm³ min^-1

Multiple Choice

What is collision theory?

• Molecules must collide in the correct orientation with enough energy to break bonds and form new bonds during a reaction.

• Molecules need enough energy to collide and react.

• Atoms constantly collide and react.

• The minimum energy needed for atoms to react

Multiple Choice

If the reactant particles collide with less than the activation energy, the particles will be rebound, and no reaction will occur.

• True

• False

Multiple Choice

With the increase in temperature, the average kinetic energy of the molecules increases, leading to a decrease in number of collisions per unit time.

• True

• False

Multiple Choice

The collisions which bring about a chemical reaction are called: 

• Consistent collisions

•  Normal collisions 

• Effective collisions 

• Magical Collisions

Multiple Choice

What factors effect rate of reaction?

• Temperature, Concentration, Pressure and Energy

• Surface Area, Concentration, Energy and Pressure

• Temperature, Pressure, Concentration and Surface area

• Pressure, Surface area, Density and Energy

Multiple Choice

Increasing the temperature of your solution will.......

• Not affect the rate of reaction.

• Speed up the rate of reaction

• Slow down the rate of reaction

Multiple Choice

If you shrink the container size that your gas substance is in what will happen?

• The reaction rate will stay the same

• The reaction rate will speed up

• The reaction rate will slow down

Multiple Choice

Why does a higher concentration increase the rate of reaction?

• it increases the amount of reactants only

• it lowers the activation energy

• it increases the energy of reactant particles

• it increases the frequency of collision

Multiple Choice

Increasing the temperature gives particles more __________.

• time

• energy

• space

• frequency

Multiple Choice

As the frequency of ________________ collision increases, the rate of reaction increases.

• time

• speed

• effective

• efficient

Multiple Choice

Why does breaking up a solid reactant increase the rate of reaction?

• it creates more solid

• it creates more energy

• it increases the total surface area

• it increases the concentration