Interpretation:
The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.
Concept introduction:
The branch of chemistry that deals with the relative rates of the
The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.
Answer to Problem 80AP
Solution:
Explanation of Solution
Given information:
The reaction between hydrogen and nitric acid, at
Experiment | Initial Rate |
||
1 | |||
2 | |||
3 |
a)The order of reaction
The order of the reaction is given by the following expression as:
Here,
Substitute the values of
Substitute the values of
Hence, the overall order of the reaction is
b) The rate constant
The rate expression for the reaction is given as follows:
Substitute the values of
Hence, the rate constant for the reaction is
c) A plausible mechanism that is consistent to rate law.
The reaction between hydrogen with nitric oxide is as follows:
The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:
The overall reaction is obtained as follows:
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Chapter 14 Solutions
EBK CHEMISTRY
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- Experiments show that the reaction of nitrogen dioxide with fluorine, 2 NO2(g) + F2(g) —* 2 FNO2(g) has the rate law Rate = *[NO2][FJ The reaction is thought to occur in two steps. Step 1: NO2(g) + F,(g) —* FNO,(g) + F(g) Step 2: NO2(g) + F(g) — FNO2(g) Show that the sum of this sequence of reactions gives the balanced equation for the overall reaction. Which step is rate determining?arrow_forwardNitrogen monoxide reacts with oxygen to give nitrogen dioxide. 2NO(g)+O2(g)2NO2(g) The rate law is [NO]/t = k[NO]2[O2], where the rate constant is 1.16 103 L2/(mol2 s) at 339oC. A vessel contains NO and O2 at 339oC. The initial partial pressures of NO and O2 arc 155 mmHg and 345 mmHg, respectively. What is the rate of decrease of partial pressure of NO (in mmHg per second)? (Hint: From the ideal gas law, obtain an expression for the molar concentration of a particular gas in terms of its partial pressure.)arrow_forwardThe following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.arrow_forward
- The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066arrow_forwardIn Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?arrow_forwardNitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?arrow_forward
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