(a)
Interpretation: The rate law of the given elementary reactions is to be determined.
Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.
To determine: The rate law for the elementary reaction,
(b)
Interpretation: The rate law of the given elementary reactions is to be determined.
Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.
To determine: The rate law for the elementary reaction,
(c)
Interpretation: The rate law of the given elementary reactions is to be determined.
Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.
To determine: The rate law for the elementary reaction,
(d)
Interpretation: The rate law of the given elementary reactions is to be determined.
Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.
To determine: The rate law for the elementary reaction,
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Chemistry: An Atoms First Approach
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- In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were obtained: Initial Concentration of Azomethane Initial Rate Exp. 1 1.13 102 M 2.8 106 M/s Exp. 2 2.26 102 M 5.6 106 M/s What is the rate law? What is the value of the rate constant?arrow_forwardAt 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?arrow_forwardNitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.arrow_forward
- The type of rate law for a reaction, either the differential rate law or the integrated rate law, is usually determined by which data is easiest to collect. Explain.arrow_forwardAmmonia decomposes when heated according to the equation NH3(g) NH2(g) + H(g) The data in the table for this reaction were collected at a high temperature. Plot In [NH3] versus time and 1/[NH3] versus time. What is the order of this reaction with respect to NH3? Find the rate constant for the reaction from the slope.arrow_forwardCompare the functions of homogeneous and heterogeneous catalysts.arrow_forward
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