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17 Nov 2019

What is the difference between the rate law of a reaction and the integrated rate law?

a.The integrated rate law excludes the rate constant.
b.Integrated rate laws always produce a linear relationship between reactant concentration and time.
c.The integrated rate law relates reactant concentration to time.

d.The integrated rate law is independent of reaction order.

Question 2

The half-life (t 1/2) of a chemical reaction is…

a. can only be determined with certainty for a first-order reaction
b.independent of concentration
c. the time required for reactant concentration to fall by one half
d. directly proportional to the rate constant k for the reaction

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Hubert Koch
Hubert KochLv2
12 Feb 2019

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Related questions

To understand how to use integrated rate laws to solve for concentration.

A car starts at mile marker 145 on a highway and drives at 55 mi/hr in the direction of decreasing marker numbers. What mile marker will the car reach after 2 hours?

This problem can easily be solved by calculating how far the car travels and subtracting that distance from the starting marker of 145.

55 mi/hr×2 hr=110 miles traveled

milemarker 145−110 miles=milemarker 35

If we were to write a formula for this calculation, we might express it as follows:

milemarker=milemarker0−(speed×time)

where milemarker is the current milemarker and milemarker0 is the initial milemarker.

Similarly, the integrated rate law for a zero-order reaction is expressed as follows:

[A]=[A]0−rate×time

or

[A]=[A]0−kt

since

rate=k[A]0=k

A zero-order reaction (Figure 1) proceeds uniformly over time. In other words, the rate does not change as the reactant concentration changes. In contrast, first-order reaction rates (Figure 2) do change over time as the reactant concentration changes.

Because the rate of a first-order reaction is nonuniform, its integrated rate law is slightly more complicated than that of a zero-order reaction.

The integrated rate law for a first-order reaction is expressed as follows:

[A]=[A]0e−kt

where k is the rate constant for this reaction.

The integrated rate law for a second-order reaction is expressed as follows:

1[A]=kt+1[A0]

where k is the rate constant for this reaction.

PART A

The rate constant for a certain reaction is k = 3.50×10−3 s−1 . If the initial reactant concentration was 0.400 M, what will the concentration be after 5.00 minutes?

Express your answer with the appropriate units.

PART B

A zero-order reaction has a constant rate of 5.00×10−4M/s. If after 75.0 seconds the concentration has dropped to 2.50×10−2M, what was the initial concentration?

Express your answer with the appropriate units.


The integrated rate law allows chemists to predict the reactantconcentration after a certain amount of time, or the time it wouldtake for a certain concentration to be reached. The integrated ratelaw for a first-order reaction is: [A]=[A]0e❝kt Now say we areparticularly interested in the time it would take for theconcentration to become one-half of its initial value. Then wecould substitute [A]02 for [A] and rearrange the equation to:t1/2=0.693k This equation calculates the time required for thereactant concentration to drop to half its initial value. In otherwords, it calculates the half-life.

Part A

What is the rate constant of a first-order reaction that takes536seconds for the reactant concentration to drop to half of itsinitial value?

Express your answer with the appropriate units.

Part B

A certain first-order reaction has a rate constant of 8.90

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