In the presence of vanadium oxide, SO,(g) reacts with an excess of oxygen to give SO3(g): VOs SO2(g) + † O2(g) → SO3(g) This reaction is an important step in the manufacture of sulfuric acid. It is observed that tripling the SO, concen- tration increases the rate by a factor of 3, but tripling the SO, concentration decreases the rate by a factor of 1.7 = V3. The rate is insensitive to the O, concentration as long as an excess of oxygen is present. (a) Write the rate expression for this reaction, and give the units of the rate constant k. (b) If [SO,] is multiplied by 2 and [SO3] by 4 but all other conditions are unchanged, what change in the rate will be observed?

In the presence of vanadium oxide, SO,(g) reacts with an excess of oxygen to give SO3(g): VOs SO2(g) + † O2(g) → SO3(g) This reaction is an important step in the manufacture of sulfuric acid. It is observed that tripling the SO, concen- tration increases the rate by a factor of 3, but tripling the SO, concentration decreases the rate by a factor of 1.7 = V3. The rate is insensitive to the O, concentration as long as an excess of oxygen is present. (a) Write the rate expression for this reaction, and give the units of the rate constant k. (b) If [SO,] is multiplied by 2 and [SO3] by 4 but all other conditions are unchanged, what change in the rate will be observed?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0088 M:5 2N,0 (g) → 2 N, (g) + 0; (g) Suppose a 400. mL flask is charged under these conditions with 200. mmol of dinitrogen monoxide. After how much time is there only 100. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 O
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Concerning the rate law, Rate = k[A]²[B], which of the following conditions will increase the rate of the reaction the most? increasing the [A] and [B] 2 times increasing the [A] 3 times while keeping the [B] unchanged increasing the [B] 3 times while keeping the [A] unchanged increasing the [B] 4 times while reducing the [A] by half increasing the [A] 4 times while reducing the [B] by half
The reaction 2 CO(g) + O₂(g) → 2 CO2(g) is described by this rate law: rate = k[CO]²[0₂] Which of the following mechanisms are consistent with this rate law? (Think carefully.) (a) CO+O₂ CO₂ + O Slow O + CO - CO₂ Fast (b) CO+O2CO3 Fast equilibrium CO3 + CO2 CO2 Slow Slow C202 +02 C204 Fast C204-2 CO2 Fast (d) 2 CO C₂02 Fast equilibrium (c) 2 CO-C₂02 C₂O2 CO₂ +O Slow O + CO → CO2 Fast
(4) Use the following experimental data to write the rate law and the rate constant for the reaction 2 NO (g) + O2 (g) = 2 NO2 (g) Experiment [NO] (M) [O2] (M) Initial rate (M/s) 1 0.0100 0.0100 0.711 x 10-2 2 0.0100 0.0400 2.84 x 10-2 3 0.0200 0.0100 2.84 x 10-2
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
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Hemoglobin molecules in blood bind oxygen and carry it to cells, where it takes part in metabolism. The binding of oxygen hemoglobin(aq) + O2(aq) – → hemoglobin · O2(aq) is first order in hemoglobin and first order in dissolved oxygen, with a rate constant of 4 × 107 L mol¯1s¯1. Calcu- late the initial rate at which oxygen will be bound to hemo- globin if the concentration of hemoglobin is 2 x 10-9 M and that of oxygen is 5 × 10-s M.
The reaction described by the equation O₂(g) + NO(g) →→→ O₂(g) + NO₂(g) has, at 310 K, the rate law rate: rate of reaction = -4 Given that [03] = 8.0 × 10−4 M and [NO] = 3.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0. k[O3 ][NO] k = 3.0 × 106 M-¹.s-¹ What is the overall order of this reaction? O 0 2 3 1 M/S
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