Chapter 16: Q16.4P (page 728)
A gas reacts with a solid presence in large chunks. Then the reaction is run again with the solid pulverized. How does the increase in the surface area of the solid affect the rate of its reaction with the gas? Explain.
The answer is,
Reaction rate increases
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The growth of Pseudomonas bacteria is modelled as a first-order process with k = 0.035 at 37°C. The initial Pseudomonas population density is cells/L.
(a) What is the population density after two h?
(b) What is the time required for the population to go from cells/ L?
Consider the following organic reaction, in which one halogen replaces another in an alkyl halide:
In acetone, this particular reaction goes to completion because KI is soluble in acetone but KBr is not. In the mechanism, I approach the carbon opposite to the Br (see Figure 16.19, with
instead of OH- ). After Br- has been replaced by and precipitates as KBr, other I ions react with the ethyl iodide by the same mechanism.
(a) If we designate the carbon bonded to the halogen as C-1, what are the shapes around C-1 and the hybridization of C-1 in ethyl iodide?
(b) In the transition state, one of the two lobes of the unhybridized 2p orbital of C-1 overlaps a p orbital of I, while the other lobe overlaps a p orbital of Br. What are the shape around C-1 and the hybridization of C-1 in the transition state?
(c) The deuterated reactant, (where D is deuterium, 2 H), has two optical isomers because C-1 is chiral. If the reaction is run with one of the isomers, the ethyl iodide is not optically active. Explain
By what factor does the rate change in each of the following cases (assuming constant temperature)?
(a) A reaction is first order in reactant A, and [A] is doubled.
(b) A reaction is second order in reactant B, and [B] is halved.
(c) A reaction is second order in reactant C, and [C] is tripled.
Reaction rate is expressed in terms of changes in the concentration of reactants andproducts. Write a balanced equation for
Rate
The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2 are reddish-brown:
Use the data below to answer the following:
(a) Determine the average rate over the entire experiment.
(b) Determine the average rate between 2.00 and 4.00 s.
(c) Use graphical methods to estimate the initial reaction rate.
(d) Use graphical methods to estimate the rate at 7.00 s.
(e) At what time does the instantaneous rate equal the average rate over the entire experiment?
Time (s) | [NOBr] (mol/L) |
0.00 | 0.0100 |
2.00 | 0.0071 |
4.00 | 0.0055 |
6.00 | 0.0045 |
8.00 | 0.0038 |
10.00 | 0.0033 |
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