The data on the table below was collected at constant temperature for the following reaction. 2A(g) + B(g) + 2C(g) → D(g) + E(g) Experiment 1 2 3 4 [A] (mol/L) 0.200 0.200 0.400 0.200 [B] (mol/L) [C] (mol/L) 0.150 0.150 0.150 0.300 1. What is the order with respect to A? [ Select] II. What is the order with respect to B? [ Select] III. What is the order with respect to C? [Select] IV. What is the overall reaction order? [Select] 0.800 0.200 0.200 0.200 Initial rate (mol/L.s) 0.500 2.00 4.00 8.00

The data on the table below was collected at constant temperature for the following reaction. 2A(g) + B(g) + 2C(g) → D(g) + E(g) Experiment 1 2 3 4 [A] (mol/L) 0.200 0.200 0.400 0.200 [B] (mol/L) [C] (mol/L) 0.150 0.150 0.150 0.300 1. What is the order with respect to A? [ Select] II. What is the order with respect to B? [ Select] III. What is the order with respect to C? [Select] IV. What is the overall reaction order? [Select] 0.800 0.200 0.200 0.200 Initial rate (mol/L.s) 0.500 2.00 4.00 8.00

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 76AE: One of the concerns about the use of Freons is that they will migrate to the upper atmosphere, where...

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The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Candle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
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Explain what is meant by the average rate of a reaction.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
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