Using the information in the table, the value of the rate constant for the reactionA(g) + 3 B(g) → C(g) + 2 D(g) isA13.4 M3 min1B0.13 min1[A], (M)[B], (M)Rate (M/min)0.3000.3000.1800.3600.0234C0.259 min10.09340.1500.1800.0234D0.26 M¹min1E0.722 M¹min1

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Answered: Using the information in the table, the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 106QRT

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Explain how a species might be part of a rate law but not part of a balanced chemical reaction.
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The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
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Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s

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Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is A 13.4 M3 min1 B 0.13 min1 [A], (M) [B], (M) Rate (M/min) 0.300 0.300 0.180 0.360 0.0234 C 0.259 min1 0.0934 0.150 0.180 0.0234 D 0.26 M¹min1 E 0.722 M¹min1