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Chapter 12: Q32 E (page 705)

Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.

Short Answer

Expert verified

The method of graphical determination is described below.

Step by step solution

01

Plotting of graph

Plots of (A), ln(A) and \(\frac{1}{{\left( A \right)}}\)versus can be done.

02

Identifying the order of the reaction

The linear plots are identified. E.g., a linear plot of (A) vs time indicates a zero-order reaction. Similarly, the plot of ln(A) vs time indicates a first-order reaction. And so on.

03

Calculation of slope and rate constant

Each plot has its own slope, which is calculated and put into the respective rate law equations.

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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

:How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate

The decomposition of acetaldehyde is a second-order reaction with a rate constant of \({\bf{4}}{\bf{.71 \times 1}}{{\bf{0}}^{{\bf{ - 8 }}}}{\bf{L mo}}{{\bf{l}}^{{\bf{ - 1}}}}{\bf{ s}}{{\bf{ }}^{{\bf{ - 1}}}}\). What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of \({\bf{5}}{\bf{.55 \times 1}}{{\bf{0}}^{{\bf{ - 4}}}}{\bf{M}}\)?

Given the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same?

\(\begin{array}{c}{\rm{(a) C}}{{\rm{l}}_2}{\rm{ + CO }} \to {\rm{ C}}{{\rm{l}}_2}{\rm{CO}}\\{\rm{rate = }}k{{\rm{(C}}{{\rm{l}}_2}{\rm{)}}^{\frac{3}{2}}}{\rm{(CO)}}\\{\rm{(b) PC}}{{\rm{l}}_3}{\rm{ + C}}{{\rm{l}}_{\rm{2}}}{\rm{ }} \to {\rm{ PC}}{{\rm{l}}_{\rm{5}}}\\{\rm{rate = }}k{\rm{(PC}}{{\rm{l}}_{\rm{3}}}{\rm{) (C}}{{\rm{l}}_{\rm{2}}}{\rm{)}}\\{\rm{(c) 2NO + }}{{\rm{H}}_{\rm{2}}}{\rm{ }} \to {\rm{ }}{{\rm{N}}_{\rm{2}}}{\rm{ + }}{{\rm{H}}_{\rm{2}}}{\rm{O}}\\{\rm{rate = }}k{\rm{(NO)(}}{{\rm{H}}_{\rm{2}}}{\rm{)}}\\{\rm{(d) 2NO + }}{{\rm{O}}_{\rm{2}}}{\rm{ }} \to {\rm{ 2N}}{{\rm{O}}_{\rm{2}}}\\{\rm{rate = }}k{{\rm{(NO)}}^{\rm{2}}}{\rm{(}}{{\rm{O}}_{\rm{2}}}{\rm{)}}\\{\rm{(e) NO + }}{{\rm{O}}_{\rm{3}}}{\rm{ }} \to {\rm{ N}}{{\rm{O}}_{\rm{2}}}{\rm{ + }}{{\rm{O}}_{\rm{2}}}\\{\rm{rate = }}k{\rm{(NO)(}}{{\rm{O}}_{\rm{3}}}{\rm{)}}\end{array}\)

The reaction of \({\bf{CO}}\) with \({\bf{C}}{{\bf{l}}_{\bf{2}}}\) gives phosgene \(\left( {{\bf{COC}}{{\bf{l}}_{\bf{2}}}} \right)\), a nerve gas that was used in World War I. Use the mechanism shown here to complete the following exercises:(fast, \({{\bf{k}}_{\bf{1}}}\) represents the forward rate constant, \({k_{ - {\bf{1}}}}\)the reverse rate constant)\({\bf{CO}}\left( g \right){\rm{ }} + {\rm{ }}{\bf{Cl}}\left( g \right) \to {\bf{COCl}}\left( g \right)\)(slow, \({k_{\bf{2}}}\) the rate constant)\({\bf{COCl}}\left( g \right){\rm{ }} + {\rm{ }}{\bf{Cl}}\left( g \right) \to {\bf{COC}}{{\bf{l}}_{\bf{2}}}\left( g \right)\)(fast,\({k_{\bf{3}}}\)the rate constant)(a) Write the overall reaction.(b) Identify all intermediates.(c) Write the rate law for each elementary reaction.(d) Write the overall rate law expression.
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