Question 1

What is the rate law for a reaction with the following stoichiometry: 2A + B -> C?

Accepted Answer

rate = k[A]²[B]

Answer

rate = k[A][B]²

Answer

rate = k[C]

Answer

rate = k[A][B]

Question 2

What is the order of a reaction if the rate constant is directly proportional to the concentration of the reactant?

Accepted Answer

1st order

Answer

2nd order

Answer

Zero order

Question 3

Based on the picture, predict the Order and Rate Law

Accepted Answer

2nd Order; Rate = k[A]²

Answer

1st Order; Rate = k[A]²

Answer

1st Order; Rate = k[A]

Answer

Zero Order; Rate = k

Answer

Zero Order; Rate = k[A]

Answer

2nd Order; Rate = k

Question 4

What is the equation for Rate of Reaction?

Accepted Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Question 5

In a study to determine the rate of the following reaction:

2NO_(g)+ O_2(g) --> 2NO_2(g)

the concentration of NO was 0.0650 M at t = 5.0 s and 0.0225 M at t = 650.0 s. What is the average rate of the reaction during this time period?

Accepted Answer

3.29 x 10^-5

Answer

3.29 x 10^-3

Answer

4.56 x 10^-3

Answer

4.56 x 10^-5

Question 6

What is the Rate Law for the following reaction?

2NO_2(g) --> NO_3(g) + NO_(g)

Accepted Answer

k[NO2]2

Answer

k= $\frac{\left[NO_3\right]\left[NO\right]}{\left[2NO\right]^2}$

Answer

k= $\frac{\left[NO_3\right]\left[NO\right]}{\left[2NO\right]^2}$

Answer

k[NO₃][NO]

Question 7

Predict the rate for experiment 4, given the other concentration/rate data provided.

(Hints: Find the experiments that don't match and divide for NO concentrations and Cl₂ concentrations. Don't forget to divide the corresponding rates. k = $\frac{rate}{\left[A\right]\left[B\right]}$ .

And Rate = $123M^{-2}s^{-1}\ x\ \left(0.00M\right)\left(0.00M\right)=Answer$ )

(Format answer as 0.00 M/s^-1)

Accepted Answer

5.04 M/s-1

Question 8

By looking at the Rate Law below:

Rate = k[FeCl₃]²[SnCl₂]

What will happen to the initial rate of the reaction if the concentration of iron(III) chloride is tripled?

Accepted Answer

It will multiply by a factor of 9.

Answer

It will triple.

Answer

It will multiply by a factor of 6.

Answer

It will remain the same.

Question 9

What Half-Life corresponds to the Integrated Rate Law for Zero Order?

Integrated Rate Law: [A]_t = -kt + [A]₀

Accepted Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Question 10

What Half-Life corresponds to the Integrated Rate Law for First Order?

Integrated Rate Law: $\ln\ \frac{\left[A\right]t}{\left[A\right]_0}=-kt$

Accepted Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Question 11

What Half-Life corresponds to the Integrated Rate Law for Second Order?

Integrated Rate Law: $\ln\ \frac{\left[A\right]t}{\left[A\right]_0}=-kt$

Accepted Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Answer

$Rate\ of\ Reaction\ =\ \frac{\Delta Concentration}{\Delta\ Time}$

Question 12

Calculate the Half-life of a first-order reaction with a rate constant of $\frac{\left[NO_3\right]\left[NO\right]}{\left[2NO\right]^2}$ ?

(Formating Hint: Just give the numbers (#####))

Accepted Answer

6.93 x 10^3

Question 13

What Factors Affect Rate?

Accepted Answer

Both Temperature and Activation Energy (E_a)

Answer

Activation Energy (E_a)

Answer

Temperature

Answer

Neither Affect Rate

Question 14

Label the parts of the Log form of the Arrhenius Equation:

$\ln\left(\frac{k_2}{k_1}\right)=-\frac{E_a}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)$

Question 15

Given in an equation, if...

$T_1=\ 308K$ , $T_2=\ 45^oC$ , $k_1=\frac{1.4\ x\ 10^{-4}\ }{s}$ , $k_2=\frac{5.0\ x\ 10^{-4}\ }{s}$ , and $R=\ 8.314\ \frac{J}{k\cdot mol}$ ....

Calculate the Activation of Energy.

(Hint: Format your answer like this, A.BCDx10^E J/mol.)

Accepted Answer

1.036x10^5 J/mol

Question 16

The Rate Determining Step is the fastest (or shortest) step in a Reaction Mechanism.

Accepted Answer

false

Answer

true

Question 17

Match the Reaction Mechanism to the corresponding step.

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