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Chapter 12: Q12.3ACYL (page 661)

The rate law for the reaction: \({{\bf{H}}_{\bf{2}}}\) (g) + 2\({\bf{NO}}\) (g) 鉄禱({\bf{N}}2{\bf{O}}\) (g) + \({{\bf{H}}_{\bf{2}}}\)O(g) has been determined to be rate = k(\({\bf{NO}}\))2 (\({{\bf{H}}_{\bf{2}}}\)). What are the orders with respect to each reactant, and what is the overall order of the reaction?

Short Answer

Expert verified

The orders with respect to each reactant order in \({\bf{NO}}\)= 2; order in \({{\bf{H}}_{\bf{2}}}\)= 1; and the overall order of the reaction overall order = 3.

Step by step solution

01

Rate of a Reaction

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

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

02

Explanation

Here m = 2 and n =1

\({\bf{rate = k(NO}}\left) {^{\bf{2}}} \right({\bf{H2)}}{\bf{.}}\)

Therefore:

The orders with respect to each reactant order in \({\bf{NO}}\) = 2; order in \({{\bf{H}}_{\bf{2}}}\)= 1; and the overall order of the reaction overall order = 3.

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Most popular questions from this chapter

How will each of the following affect the rate of the reaction:

\({\bf{CO}}\left( {\bf{g}} \right){\bf{ + \;N}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {{\bf{O}}_{\bf{2}}}{\bf{\;}}\left( {\bf{g}} \right){\bf{ + NO}}\left( {\bf{g}} \right)\) if the rate law for the reaction is rate = \({\bf{k(NO}}{}_{\bf{2}}{\bf{)(CO)}}\)?

  1. Increasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.1 atm to 0.3 atm
  2. Increasing the concentration of CO from 0.02 M to 0.06 M.

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 \({\bf{5}}{\bf{.8 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}{\bf{ L}}{{\bf{ }}^{\bf{2}}}{\bf{ mo}}{{\bf{l}}^{{\bf{ - 2}}}}{\bf{ s}}{{\bf{ }}^{{\bf{ - 1}}}}\).

Use the PhET Reactions & Rates interactive simulation to simulate a system. On the 鈥淪ingle collision鈥� tab of the simulation applet, enable the 鈥淓nergy view鈥� by clicking the 鈥�+鈥� icon. Select the first A + BC鉄禔B + C reaction (A is yellow, B is purple, and C is navy blue). Using the 鈥渟traight shot鈥� default option, try launching the A atom with varying amounts of energy. What changes when the Total Energy line at launch is below the transition state of the Potential Energy line? Why? What happens when it is above the transition state? Why?

When every collision between reactants leads to a reaction, what determines the rate at which the reaction occurs?

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鈥�30%. Women metabolize alcohol a little more slowly than men:

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