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Chapter 12: Q15E (page 703)

How much and in what direction will each of the following effect the rate of the reaction:

CO(g) + \({\bf{NO}}{}_{\bf{2}}\) (g)鉄� \({\bf{CO}}{}_{\bf{2}}\) (g) + NO(g) if the rate law for the reaction is rate =\({\bf{k(NO}}{}_{\bf{2}}{{\bf{)}}^{\bf{2}}}{\bf{a}}\)?

  1. Decreasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.50 atm to 0.250 atm.
  2. Increasing the concentration of CO from 0.01 M to 0.03 M.

Short Answer

Expert verified
  1. Decreasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.50 atm to 0.250 atm is factor 4
  2. Increasing the concentration of CO from 0.01 M to 0.03 M. is not affect the rate of reaction

Rate law predict the relationship between rate of reaction and concentration of reaction.

Step by step solution

01

Rate of reaction

\(\frac{{{\bf{rate(R}}{}_{\bf{1}}{\bf{)}}}}{{{\bf{rate(R}}{}_2{\bf{)}}}}{\bf{ = }}\frac{{{\bf{k(0}}{\bf{.25NO}}{}_{\bf{2}}{{\bf{)}}^{\bf{2}}}}}{{{\bf{k(0}}{\bf{.50NO}}{}_{\bf{2}}{{\bf{)}}^{\bf{2}}}}}{\bf{ = }}\frac{{{\bf{0}}{\bf{.0625}}}}{{{\bf{0}}{\bf{.25}}}}{\bf{ = }}\frac{{\bf{1}}}{{\bf{4}}}\)

Here rate (\({\bf{R}}{}_{\bf{1}}\)) is four time large from rate (\({\bf{R}}{}_2\)). Pressure reduces the rate by factor of 4.

02

Rate of reaction

Carbon monoxide does not affect to rate law. So, it does not change the rate of reaction.

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Most popular questions from this chapter

In a transesterification reaction, a triglyceride reacts with an alcohol to form an ester and glycerol. Many students learn about the reaction between methanol (\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\)) and ethyl acetate (\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}\)) as a sample reaction before studying the chemical reactions that produce biodiesel:

\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH + C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}{\bf{ - - - C}}{{\bf{H}}_{\bf{3}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}{\bf{ + C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OH}}\).The rate law for the reaction between methanol and ethyl acetate is, under certain conditions, determined to be: rate =\(k\left( {{\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH }}} \right)\). What is the order of reaction with respect to methanol and ethyl acetate, and what is the overall order of reaction?

The rate constant for the first-order decomposition at 45 掳C of dinitrogen pentoxide, N2O5, dissolved in chloroform, \({\bf{CHC}}{{\bf{l}}_3}\), is 6.2 脳 10鈭�4 min鈭�1.

\({\bf{2}}{{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}} \to {\bf{4N}}{{\bf{O}}_{\bf{2}}}{\bf{ + }}{{\bf{O}}_{\bf{2}}}\)

What is the rate of the reaction when \({{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}}{\bf{\; = 0}}{\bf{.40 M}}\)

Use the provided initial rate data to derive the rate law for the reaction whose equation is: \({\bf{OC}}{{\bf{l}}^ - }\)(aq) + \({{\bf{I}}^ - }\)(aq) 鉄禣I鈭�(aq) +\({\bf{C}}{{\bf{l}}^ - }\)(aq)

Trial

(\({\bf{OC}}{{\bf{l}}^ - }\)) (mol/L)

(\({{\bf{I}}^ - }\)) (mol/L)

Initial Rate (mol/L/s)

1.

0.0040

0.0020

0.00184

2.

0.0020

0.0040

0.00092

3.

0.0020

0.0020

0.00046

Determine the rate law expression and the value of the rate constant k with appropriate units for this reaction.

In the PhET Reactions & Rates (http://openstaxcollege.org/l/16PHETreaction) interactive, on the Many Collisions tab, set up a simulation with 15 molecules of A and 10 molecules of BC. Select 鈥淪how Bonds鈥� under Options.

  1. Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow?
  2. Click 鈥淧ause鈥� and then 鈥淩eset All,鈥� and then enter 15 molecules of A and 10 molecules of BC once again. Select 鈥淪how Bonds鈥� under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction

A study of the rate of dimerization of \({{\bf{C}}_{\bf{4}}}{{\bf{H}}_{\bf{6}}}\) gave the data shown in:

\({\bf{2}}{{\bf{C}}_{\bf{4}}}{{\bf{H}}_{\bf{6}}} \to {{\bf{C}}_{\bf{8}}}{{\bf{H}}_{{\bf{12}}}}\)

  1. Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s.
  2. Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus (\({{\bf{C}}_{\bf{4}}}{{\bf{H}}_{\bf{6}}}\)). What are the units of this rate?

(c) Determine the average rate of formation of \({{\bf{C}}_{\bf{8}}}{{\bf{H}}_{{\bf{12}}}}\) at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
See all solutions

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