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Chapter 12: Q21E (page 703)

Alcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 25–30%. Women metabolize alcohol a little more slowly than men:

Determine the rate equation, the rate constant, and the overall order for this reaction.

Short Answer

Expert verified

Rate does not change with change concentration that’s why; it is zero order of the reaction.

The rate equation will be as follows

\(Rate = k{\left( {concentration} \right)^0}\)

\({\rm{Rate constant}}\left( k \right) = 2.0 \times {10^{ - 2}}\,{\rm{mol}}\,{{\rm{L}}^{{\rm{ - 1}}}}{{\rm{h}}^{{\rm{ - 1}}}}\)

Step by step solution

01

Metabolic reactions

In human the end product of alcohol metabolism is acetaldehyde, both in liver and brain by the action of enzymes alcohol dehydrogenase and cytochrome p450 respectively. Acetaldehyde is highly unstable, reactive and cytotoxic, which can cause severe liver damage.

02

Rate of reaction and concentration

The rate law for a chemical reaction is an expression that provides a relationship between the rate of the reaction and the concentration of the reactants participating in it. It can also be a second-order reaction.

An instantaneous rate of change is the change in the rate at a particular instant.

From the given table it is clear that rate is not changing with change in concentrations that means rate of reaction is independent of concentration of reactant which is the condition of zero order reaction.

Zero order reaction is a chemical reaction in which the rate of reaction is constant and independent of the concentration of reacting substance.

\(\begin{aligned}{}{\bf{Rate = k}}\\{\bf{k = 2}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}{\bf{mol}}{{\bf{L}}^{{\bf{ - 1}}}}{{\bf{h}}^{{\bf{ - 1}}}}\end{aligned}\)

Here rate does not change with a change in concentration so, it is zero order of the reaction.

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Most popular questions from this chapter

Fluorine-18 is a radioactive isotope that decays by positron emission to form oxygen-18 with a half-life of 109.7 min. (A positron is a particle with the mass of an electron and a single unit of positive charge; the equation is (\({_{{\bf{518}}}^{\bf{9}}}{\bf{F}}\)⟶\({_{{\bf{18}}}^{\bf{8}}}{\bf{O + e - }}\).) Physicians use\(^{{\bf{18}}}{\bf{F}}\)to study the brain by injecting a quantity of fluoro-substituted glucose into the blood of a patient. The glucose accumulates in the regions where the brain is active and needs nourishment.

(a) What is the rate constant for the decomposition of fluorine-18?

(b) If a sample of glucose containing radioactive fluorine-18 is injected into the blood, what percent of the radioactivity will remain after 5.59 h?

(c) How long does it take for 99.99% of the\(^{{\bf{18}}}{\bf{F}}\)to decay?

Thefollowingdatahave been determined for the reaction: \({{\bf{I}}^{\bf{ - }}}{\bf{ + OC}}{{\bf{l}}^{\bf{ - }}} \to {\bf{I}}{{\bf{O}}^{\bf{ - }}} + {\bf{C}}{{\bf{l}}^{\bf{ - }}}\)

1

2

3

\({{\bf{(}}{{\bf{I}}^{\bf{ - }}}{\bf{)}}_{{\bf{initial}}}}\)(M)

0.10

0.20

0.30

\({{\bf{(OC}}{{\bf{l}}^{\bf{ - }}}{\bf{)}}_{{\bf{initial}}}}\)(M)

0.050

0.050

0.010

Rate(mol/l/s)

\({\bf{3}}{\bf{.5*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

\({\bf{6}}.{\bf{2*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

\({\bf{1}}.{\bf{83*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

Determine the rate equation and the rate constant for this reaction.

What is the half-life for the first-order decay of phosphorus-32?\(_{{\bf{15}}}^{{\bf{32}}}{\bf{P}} \to _{{\bf{16}}}^{{\bf{32}}}{\bf{S + }}{{\bf{e}}^{\bf{ - }}}\)The rate constant for the decay is\({\bf{4}}{\bf{.85 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}{\bf{da}}{{\bf{y}}^{{\bf{ - 1}}}}\).

For each of the following pairs of reaction diagrams, identify which of the pair iscatalyzed:

Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation:\({{\bf{H}}_{\bf{2}}}{\bf{(g) + 2NO(g)}} \to {{\bf{N}}_{\bf{2}}}{\bf{O(g) + }}{{\bf{H}}_{\bf{2}}}{\bf{O}}\).Determine the rate law, the rate constant, and the orders with respect to each reactant from the following data:
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