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Chapter 16: Q16.25 P (page 729)

By what factor does the rate change in each of the following cases (assuming constant temperature)?

(a) A reaction is first order in reactant A, and [A] is doubled.

(b) A reaction is second order in reactant B, and [B] is halved.

(c) A reaction is second order in reactant C, and [C] is tripled.

Short Answer

Expert verified
  1. When the reaction is doubled, the rates increase by a factor of 2.
  2. When the reaction is halved, the rate reduces by a factor of 4.
  3. When the reaction is tripled, the rate rises by a factor of 9.

Step by step solution

01

(a) When the reaction is doubled

For reactant A, write the rate law for the reaction in a first-order:

rate=kA1

When the concentration of the reactant doubles, write a new rate rule for the reaction:

rate=k2脳A1=2脳kA1

As a result, the rates increase by a factor of 2.

02

(b) When the reaction is halved

For reactant B, write the rate law for the reaction in a second order:

rate=kB2

When the concentration of the reactant is half, write the following revised rate law for the reaction:

rate=k12脳B2=14脳kB2

As a result, the rate reduces by a factor of 4.

03

 Step 3: (c) When the reaction is triple

For reactant C, write the rate rule for the reaction in a second order:

rate=kC2

Write a new rate rule for the reaction when the reactant concentration is tripled:

rate=k3脳C2=9脳kC2

As a result, the rate rises by a factor of 9.

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Most popular questions from this chapter

Question: Reaction rate is expressed in terms of changes in concentration of reactants and products. Write a balanced equation for

Rate=-鈭�[CH4]鈭唗=12鈭�[O2]鈭唗=12鈭�[H2O]鈭唗=-鈭�[CO2]鈭唗

The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2 are reddish-brown:

2NOBr(g)鈫�2NO(g)+Br2(g)

Use the data below to answer the following:

(a) Determine the average rate over the entire experiment.

(b) Determine the average rate between 2.00 and 4.00 s.

(c) Use graphical methods to estimate the initial reaction rate.

(d) Use graphical methods to estimate the rate at 7.00 s.

(e) At what time does the instantaneous rate equal the average rate over the entire experiment?

Time (s)

[NOBr] (mol/L)

0.00

0.0100

2.00

0.0071

4.00

0.0055

6.00

0.0045

8.00

0.0038

10.00

0.0033

An atmospheric chemist fills a container with gaseous N2O5 to a pressure of 125 kPa, and the gas decomposes toNO2 and O2. What is the partial pressure of PNO2, (in kPa), when the total pressure is 178 kPa?

The formation of ammonia is one of the most important processes in the chemical industry:

N2(g)+3H2(g)鈫�2NH3(g)


Express the rate in terms of changes in[N2], [H2], and[NH3].

Consider the following organic reaction, in which one halogen replaces another in an alkyl halide:

CH3CH2Br+Kl鈫�CH3CH2l+KBr

In acetone, this particular reaction goes to completion because KI is soluble in acetone but KBr is not. In the mechanism, I approach the carbon opposite to the Br (see Figure 16.19, withl-

instead of OH- ). After Br- has been replaced by l-and precipitates as KBr, other I ions react with the ethyl iodide by the same mechanism.

(a) If we designate the carbon bonded to the halogen as C-1, what are the shapes around C-1 and the hybridization of C-1 in ethyl iodide?

(b) In the transition state, one of the two lobes of the unhybridized 2p orbital of C-1 overlaps a p orbital of I, while the other lobe overlaps a p orbital of Br. What are the shape around C-1 and the hybridization of C-1 in the transition state?

(c) The deuterated reactant, CH3CHDBr(where D is deuterium, 2 H), has two optical isomers because C-1 is chiral. If the reaction is run with one of the isomers, the ethyl iodide is not optically active. Explain
See all solutions

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