(ii). Identify all reaction intermediates. (iii). Write the rate law for the rate-determining step. (iv). Show an equation for the rate of the overall reaction in terms of the concentrations of the reactants.

(ii). Identify all reaction intermediates. (iii). Write the rate law for the rate-determining step. (iv). Show an equation for the rate of the overall reaction in terms of the concentrations of the reactants.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 32P

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Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

Kindly answer question a ii, iii & iv

(a). Consider the following mechanism for the reaction of nitric oxide and hydrogen:
k1
2 NO(g)
N2O2(g)
k.1
Fast
k2
N2O2(g) + H2(g)
N20(g) + H2O(9)
Slow rate-determining
k3
N20(g) + H2(g)
N2(g) + H2O(g)
Fast
The first step, which is reversible has a constant of ki for the forward reaction
and k-1 for the reverse reaction. The forward and the reverse reactions in step
1 occur in the same rate, and both are fast compared with step 2, the rate-
determining step.
(i). Write an equation for the overall reaction.
(ii). Identify all reaction intermediates.
(iii). Write the rate law for the rate-determining step.
(iv). Show an equation for the rate of the overall reaction in terms of the
concentrations of the reactants.
(b). Explain the relationship between the coefficient in a balanced chemical
equation for an overall reaction and the exponents in the rate law.
(c). The widely used solvent ethyl acetate undergoes the following reaction in basic
solution:
CH3CO2C2H5(aq) + OH (aq)
CH:CO2 (аq) + C2H5ОН(аq)
The rate of this reaction increases by a factor of 7.3 on raising the temperature
from 16 °C to 46 °C. Calculate the value of the activation energy in kJ mol-1.

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