Question 1

For the reaction: 3BrO-(aq) --> BrO3-(aq) + 2Br-(aq)

[BrO]initial is 0.60 M. 70 seconds later [BrO] is 0.12 M. What is the rate of change of [BrO] in M/s? (The brackets, [ ], indicate concentration, that is, molarity (M) or moles/liter.) Explanation

Notice that the rate of change of a reactant is negative because it is being used up. Question 2

Under a different set of conditions, the initial concentration of Br- is 0.00 M. 81 seconds later it is 0.82 M. What is the rate of change of Br- in M/s? Explanation

Notice that the rate of change of a product is positive because it is being produced. Question 3

Under a different set of conditions, the initial concentration of BrO3- is 0.23 M. 14 seconds later it is 0.83 M. What is the rate of change of BrO3- in M/s? Explanation

Notice that the rate of change of a product is positive because it is being produced.

Question 4

Still for the reaction: 3BrO-(aq) --> BrO3-(aq) + 2Br-(aq), what is the rate of reaction in M/s, if Δ[BrO]/Δt = -0.074 M/s?

Help: Rate of reaction Explanation

We are given the rate of change of [BrO].  Because the chemical equation has 3 moles of BrO, we must divide by 3 to get the rate of reaction. Note that the rate of reaction is always positive.

Question 5

Under a different set of conditions Δ[BrO3- ]/Δt = 0.029 M/s. What is the rate of reaction in M/s? Explanation

In this case, the coefficient of [BrO3-] is 1.  Therefore:

Δ[BrO3- ]/Δt = Rate of reaction = .029

Note that the rate of reaction is always positive.

Question 6

Under a different set of conditions Δ[Br]/Δt = 0.035 M/s. What is the rate of reaction in M/s? Explanation Note that the rate of reaction is always positive.

Question 7

If Δ[BrO3- ]/Δt = 0.010 M/s. What is Δ[Br]/Δt in M/s? Reminder, the rate of change [BrO3- ] is Δ[BrO3- ]/Δt.

Help: Rate of change of reactants and products Explanation

Once again, take a look at the coefficients (molar amounts) in the chemical reaction to help you solve this one.

If Δ[BrO3- ]/Δt = 0.010 M/s,

then Δ[Br]/Δt = 0.010 x 2 = 0.020

Question 8

If Δ[BrO3]/Δt = 0.024 M/s. What is [BrO]/Δt in M/s? Explanation

Note that [BrO]/Δt is negative, because BrO- is a reactant. Question 9

The rate of change of [B] is -0.243 M/min. What is the rate of reaction for the following reaction in M/min?

2A + 5B → 3C + 7D Explanation

(-.0243) / -5 = .0486

Question 10

Under a different set of conditions, the rate of change of [C] is 0.162 M/min. What is the rate of change of [D] in M/min? Hint given in feedback Explanation

Hint, if a = b and b = c, then a = c.

Specifically, what is the rate of reaction using [C] and what is the rate using [D]? Set the rate using [C] = the rate using [D] and solve for the rate of change of [D]. Question 11

If the rate of change of [C] is 0.149 M/min. What is the rate of change of [A] in M/sHint given in feedback' Explanation

Hint. What is the rate of reaction using [C] and what is the rate using [A]? Set the rate using [C] = the rate using [A] and solve for the rate of change of [A]. Check: is the rate of change of [A] positive or negative?

Finally, units for rate of change of [A] are M/s not M/min. (1/min) = (1/min)(1 min/60 s). Question 12

For the reaction 2A +3B → C + 4D

The rate of reaction = k[A]0.5[B]2

Which of the following statements are true?

Select one or more:   Explanation

To determine order of a particular reactant, look at its superscript.

To determine overall reaction rate order, find the sum of superscripts.

Question 13

For a new reaction with reactant "A", suppose the rate of reaction is 0.04 M/sec when [A] = 0.23 M. The concentration of A is doubled to 0.46 M. Match the rate of reaction to the reaction order.

 Rate is still 0.04 M/s Answer 1Choose...zero orderone-half ordersecond orderfirst order Rate is 0.04 x 20.5 = 0.057 M/s Answer 2Choose...zero orderone-half ordersecond orderfirst order Rate is 0.04 x 21 = 0.08 M/s Answer 3Choose...zero orderone-half ordersecond orderfirst order Rate is 0.04 x 22 = 0.16 M/s Answer 4Choose...zero orderone-half ordersecond orderfirst order Explanation

Here we are essentially comparing the relative amount of change in concentration (∆[A]) to the relative amount of change in reaction rate in order to find the reaction order.

Note that K (rate constant) cancels out in each equation.    Question 14

For the reaction 2NO2(g) → 2NO(g) + O2(g)
the following experimental data was obtained for the rate:

Run
[NO2] (M)
Rate (M/s)
1
0.16
0.27
2
0.32
1.08
3
0.64
4.32

What is the reaction rate order? Hint given in feedback.

Select one: Explanation

Hint, what happens to the reaction rate when the reactant concentration is doubled? Question 15

What is k? Hint given in feedback Explanation

Substitute the data from one of the runs into the appropriate equation and solve for k.

For zero-order, the rate of reaction = k[NO2]0 = k.
For first-order, the rate of reaction = k[NO2]1
For one half-order, the rate of reaction = k[NO2]0.5
For second-order, the rate of reaction = k[NO2]2 Question 16

What are the units of k?

Select one: Explanation Question 17

What is the rate when [NO2] = 0.121 M?

Hint given in feedback Explanation

Use the rate equation for the correct order with the k that you determined. Question 18

For the reaction 2H2O2(aq) → 2H2O(l) + O2(g)
the following experimental data was obtained for the rate:

Run
[H2O2] (M)
Rate (M/s)
1
0.043
0.19
2
0.065
0.29
3
0.086
0.38

What is the reaction rate order? Hint given in feedback

Select one: Explanation

It is easiest to use the first and third run to determine the order. Question 19

What is k? Hint given in feedback Explanation

Substitute the data from one of the runs into the appropriate equation and solve for k.

For zero-order, the rate of reaction = k[H2O2]0 = k.
For first-order, the rate of reaction = k[H2O2]1
For one half-order, the rate of reaction = k[H2O2]0.5
For second-order, the rate of reaction = k[H2O2]2 Question 20

What are the units of k?

Select one: Question 21

What is the rate when [H2O2] = 0.082 M?

Hint given in feedback Explanation

Use the rate equation for the correct order with the k that you determined. Question 22

For the reaction 2A(g) + 3B(g) → C(g) + 2D(g)
the following experimental data was obtained for the rate:

Run
[A] (M)
[B] (M)
Rate (M/min)
1
0.01
0.2
2.2
2
0.01
0.4
4.4
3
0.02
0.4
8.8

The rate of reaction = kAxBy. What is x? Hint given in feedback Explanation

Hint: Notice that in run #2 and #3 the concentration of B does not change. So, it does not change the rate. Therefore, you can use these runs to find the order of the reaction with respect to A. In what two runs is the concentration of A the same? Use these runs to find the order of the reaction with respect to B.

From run 2 to 3, [A] doubles.  Rate also doubles.  This means that x=1.

Question 23

What is y? Explanation

From run 1 to 2, [B] doubles.  Rate also doubles.  This means that y=1.

Question 24

What is k? Explanation

Plug in values for a single run, as well as the x and y values determined above to solve for k.

Question 25

What are the units of k?

Select one: Question 26

What is the rate when [A] = 0.043 M and [B] = 0.038 M?

Hint given in feedback Explanation

Use the rate equation for the correct order with the k that you determined.

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Find out what the next lecture will be about and review the material ahead of time.

Imagine already knowing the material that the professor will be going over–this can make a huge difference in your retention and success, not to mention make you look like a stud when you know all the answers ;)