Consider this reaction: 2H3PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. (93.8 M¹-s −¹)[H₂PO4]² rate= Suppose a vessel contains H₂PO4 at a concentration of 0.270M. Calculate how long it takes for the concentration of H3PO4 to decrease to 22.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. X

Consider this reaction: 2H3PO4 (aq) → P₂O5 (aq) + 3H₂O (aq) At a certain temperature it obeys this rate law. (93.8 M¹-s −¹)[H₂PO4]² rate= Suppose a vessel contains H₂PO4 at a concentration of 0.270M. Calculate how long it takes for the concentration of H3PO4 to decrease to 22.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. X

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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For the reaction: 3X (g) + 5Y (g) a b. →2Z (g) + 4L (g) Express the rate of the reaction in terms of the change in concentration of each reactant and product with time. + ✪ [X] is decreasing by ◆ = When [Z] is increasing at 0.16 mol/L.s, show how fast is [X] decreasing. + unit is ◆
7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?
The reaction 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results: Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s) 1 0.00542 0.00542 0.341 2 0.00542 0.0108 0.679 3 0.0108 0.00542 0.679 4 0.0108 0.0108 1.35 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)] Rate = k [HBr(g)] [O2(g)]2 Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HBr(g) is 0.00861 M and that of O2(g) is 0.0123 M if the temperature is the same as that used to obtain the data shown above? _________M/s
A student suspects that the nitrate ion (NO3−), rather than the Cu2+ ion, is the active species in the Cu(NO3)2 catalyst. He devises a second experiment to test his hypothesis, using KNO3 as a potential catalyst. If the student's hypothesis is correct, what should he observe when KNO3 is added to the reaction? Any changes are observed relative to an identical un-catalyzed reaction. a. The rate of the reaction will decrease b. The rate of the reaction will increase c. There will be no change in the rate of the reaction
For the reaction, 2NOBr(g) ⇋ 2NO(g) + Br2(g) The rate of the reaction was 22.3 mol NOBr/L/h when the initial NOBr concentration was 6.2 mol NOBr/L. What is the rate constant of the reaction?
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
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Consider the reaction: 2NO(g) + O₂(g) 2 NO₂ (g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of -0.054 M S
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
The conversion of cyclopropane to propene (Example 14.5) occurs with a first-orderrate constant of 2.42 ×10−2 h−1. How long will it take for the concentration ofcyclopropane to decrease from an initial concentration of 0.080 mol/L to 0.020 mol/L?
Nitrite ion reacts with ozone in aqueous solution, producing nitrate ion and oxygen:NO−2 (aq)+O3 (g)NO−3 (aq)+O2 (g)The following data were collected for this reaction at 298 K. Calculate the average reaction rate between 0 and 100 μs (microseconds) and between 200 and 300 μs. Time (μs) [O3] (M) 0 1.113x10-2 100 9.992x10-3 200 8.797x10-3 300 8.183x10-3 Average reaction rate between 0 and 100 μs = x 10 M/μs