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Chapter 12: Q12.7CYL (page 670)

Graph the following data to determine whether the reaction A鉄禕 + C is first order.

Trial

Time(s)

(A)

1

4.0

0.220

2

8.0

0.144

3

12.0

0.110

4

16.0

0.088

5

20.0

0.074

Short Answer

Expert verified

The graph plot of ln(A) vs. t is not a straight line.

Step by step solution

01

Rate of a Reaction

The rate of reaction may be defined as the speed of the reactant reacting to give obtain in a particular reaction at a particular time. The concentration of the reactant and product are represented into mole/L.

Rate\({\bf{ = }}\,{\bf{ k}}{\left( {\bf{A}} \right)^{\bf{m}}}{\left( {\bf{B}} \right)^{\bf{n}}}^{}\)

02

First Order Reaction

The rate equation consists of initial concentration \({\left( {\bf{A}} \right)_{\bf{0}}}\)and the concentration \({\left( {\bf{A}} \right)_{\bf{t}}}\)present after any given time t can be derived for a first-order reaction. Rearrange the integrated standard linear equation format:

\({\bf{ln}}\left( {\bf{A}} \right){\bf{ = }}\left( {{\bf{ - k}}} \right)\left( {\bf{t}} \right){\bf{ + ln}}{\left( {\bf{A}} \right)_{\bf{t}}}\)

y = mx + b

03

Graph

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Most popular questions from this chapter

In terms of collision theory, to which of the following is the rate of a chemical reaction proportional?

(a) the change in free energy per second

(b) the change in temperature per second

(c) the number of collisions per second

(d) the number of product molecules

The annual production of \({\bf{HN}}{{\bf{O}}_{\bf{3}}}\) in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel.

\(\begin{align}\left( a \right){\bf{ }}4N{H_3}{\bf{ }}\left( g \right){\bf{ }} + {\bf{ }}5{O_2}{\bf{ }}(g) \to 4NO\left( g \right){\bf{ }} + {\bf{ }}6{H_2}O\left( g \right)\\\left( b \right){\bf{ }}2NO\left( g \right){\bf{ }} + {\bf{ }}{O_{2{\bf{ }}}}(g) \to 2N{O_{2{\bf{ }}}}\left( g \right)\\\left( c \right){\bf{ }}3N{O_2}{\bf{ }}\left( g \right){\bf{ }} + {\bf{ }}{H_2}O(l) \to 2HN{O_3}(aq) + NO(g)\end{align}\)

The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in \({{\bf{O}}_{\bf{2}}}\), what is the rate of formation of \({\bf{N}}{{\bf{O}}_{\bf{2}}}\) when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M? The rate constant for the reaction is \({\bf{5}}{\bf{.8 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}{\bf{ L}}{{\bf{ }}^{\bf{2}}}{\bf{ mo}}{{\bf{l}}^{{\bf{ - 2}}}}{\bf{ s}}{{\bf{ }}^{{\bf{ - 1}}}}\).

Atomic chlorine in the atmosphere reacts with ozone in the following pair of elementary reactions:

\({\bf{Cl + \;O3}}\left( {\bf{g}} \right){\bf{ - - - ClO}}\left( {\bf{g}} \right){\bf{ + \;O2}}\left( {\bf{g}} \right)\)(rate constant k1 )

\({\bf{ClO}}\left( {\bf{g}} \right){\bf{ + O - - - Cl}}\left( {\bf{g}} \right){\bf{ + \;O2}}\left( {\bf{g}} \right)\)(rate constant k2 )

Determine the overall reaction, write the rate law expression for each elementary reaction, identify any intermediates, and determine the overall rate law expression.

From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2X鉄禮 + Z

Time(s)

5.0

10.0

15.0

20.0

25.0

30.0

35.0.

40.0

(X)(M)

0.0990

0.0497

0.0332

0.0249

0.0200

0.0166

0.0143

0.0125

Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces:

\(\begin{aligned}{l}_{{\bf{15}}}^{{\bf{32}}}{\bf{P}} \to _{{\bf{16}}}^{{\bf{32}}}{\bf{S + }}{{\bf{e}}^{\bf{ - }}}\\{\bf{rate = 4}}{\bf{.85 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}\,{\bf{da}}{{\bf{y}}^{{\bf{ - 1}}}}{{\bf{(}}^{{\bf{32}}}}{\bf{p)}}\end{aligned}\)

What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of \({\bf{0}}{\bf{.0033 M}}\)?

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