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Chapter 16: Q16.66P (page 731)

Explain why the coefficients of an elementary step equal the reaction orders of its rate law but those of an overall reaction do not.

Short Answer

Expert verified

When two molecules collide, an elementary step is created in a single step. The rate of an elementary step is proportional to the product of the concentrations of the reactants with the same exponents (order) as the stoichiometric coefficients in the equation for this step. The complete reaction may have a number of such stages with varying speeds. On the other hand, the speed is computed using the slowest step. As a result, the reaction orders of its rate law do not necessarily match the stoichiometric coefficients of the overall equation.

Step by step solution

01

What is the reaction of an elementary?

A chemical reaction in which one or more chemical species react directly to create products in a single reaction step and with a single transition state is known as an elementary reaction.

02

Why do the coefficients of an elementary step match the reaction orders of its rate law

The collision of two molecules creates an elementary step in a single step. The product of the concentrations of the reactants with the same exponents (order) as the stoichiometric coefficients in the equation for this step is proportional to the rate of an elementary step. A number of such phases with varying speeds may be included in the total reaction. However, the pace is calculated using the slowest step. As a result, the reaction orders of its rate law do not always match the overall equation's stoichiometric coefficients.

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Most popular questions from this chapter

What is the central idea of collision theory? How does this idea explain the effect of concentration on reaction rate?

Ina kinetics experiment, a chemist places crystals of iodine in a closed reaction vessel, introduces a given quantity of hydrogen gas, and obtains data to calculate the rate of hydrogen iodide formation. In a second experiment, she uses the same amounts of iodine and hydrogen, but first warms the flask to 130 degrees Celsius, a temperature above the sublimation point of iodine. In which of these experiments does the reaction proceed at a higher rate? Explain.

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

Give two reasons to measure initialrates in a kinetic study.

Question:Many drugs decompose in blood by a first-order process.

(a) Two tablets of aspirin supply 0.60 g of the active compound. After 30 min, this compound reaches a maximum concentration of 2 mg/100 mL of blood. If the half-life for its breakdown is 90 min, what is its concentration (in mg/100 mL) 2.5 h after it reaches its maximum concentration?

(b) For the decomposition of an antibiotic in a person with a normal temperature (98.6掳F),k=3.1脳10-5s-1; for a person with a fever at 101.9掳F, k=3.9脳10-5s-1. If the person with the fever must take another pill when of the first pill has decomposed, how many hours should she wait to take a second pill? A third pill? (Assume the pill is effective immediately.)

(c) Calculate Ea for decomposition of the antibiotic in part (b).
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