(a)
Interpretation:
The determination of complete rate law from the data is possible or not has to be examined.
Concept Introduction:
The relationship between rate and initial concentration of reactant is described by rate law. It is an experimentally determined equation and cannot be found out theoretically from the stoichiometry of the reactants and products.
Where,
(b)
Interpretation:
The rate law has to be determined by assuming that the rate does not depend on the concentration of hydroxide ion.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Rate constant has to be calculated by assuming that the rate does not depend on the concentration of hydroxide ion.
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The initial
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
The rate of the reaction has to be calculated when the concentration of
Concept Introduction:
Refer to part (a).
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Chapter 11 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- The 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_forwardDefine stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forwardWhen boron trifluoride reacts with ammonia, the following reaction occurs: BF3(g)+NH3(g)BF3NH3(g)The following data are obtained at a particular temperature: (a) What is the order of the reaction with respect to BF3, NH3, and overall? (b) Write the rate expression for the reaction. (c) Calculate k for the reaction. (d) When [ BF3 ]=0.533M and NH3=0.300M, what is the rate of the reaction at the temperature of the experiment?arrow_forward
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