Chapter 12: Q69 E (page 710)
Ingeneral, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A + B⟶C? Can we predict the effect if the reaction is known to be an elementary reaction?
The effect depends on the type of reaction.
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2X⟶Y + 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 |
Usethe data provided to graphically determine the order and rate constant of the following reaction: \({\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{C}}{{\bf{l}}_{\bf{2}}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{ + C}}{{\bf{l}}_{\bf{2}}}\)
Time(hr) | 0 | 5.00*\({\bf{1}}{{\bf{0}}^{\bf{3}}}\) | 1.00*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\) | 1.50*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\) | 2.50*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\) | 3.00*104 | 4.00*104 |
\({\bf{(S}}{{\bf{O}}_{\bf{2}}}{\bf{C}}{{\bf{l}}_{\bf{2}}}{\bf{)}}\)(M) | 0.100 | 0.0896 | 0.0802 | 0.0719 | 0.0577 | 0.0517 | 0.0415 |
For each of the following pairs of reaction diagrams, identify which of the pairs iscatalyzed:
What is the rate equation for the elementary termolecular reaction A + 2B⟶products? For 3A⟶products?
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 \({\bf{5}}{\bf{.8 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}{\bf{ L}}{{\bf{ }}^{\bf{2}}}{\bf{ mo}}{{\bf{l}}^{{\bf{ - 2}}}}{\bf{ s}}{{\bf{ }}^{{\bf{ - 1}}}}\).
What do you think about this solution?
We value your feedback to improve our textbook solutions.
