The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first- order reaction: 4PH3(g)P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. Calculate the first-order rate constant for the reaction: -1 Calculate the time required for 95.0 percent of the phosphine to decompose:

The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first- order reaction: 4PH3(g)P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. Calculate the first-order rate constant for the reaction: -1 Calculate the time required for 95.0 percent of the phosphine to decompose:

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...

See similar textbooks

Similar questions

A student obtained the following data for the gas phase decomposition of hydrogen peroxide at 400 °C. H₂O₂(g) H₂O(g) + 2 O₂(g) [H₂0₂], M seconds 0.134 0 6.70x10-² 14.2 ◊ 3.35x10-2 42.7 (1) What is the half-life for the reaction starting at t=0 s? What is the half-life for the reaction starting at t=14.2 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? 1.68x10-2 99.2 (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction? S M-¹S-1
The following data were collected for the reaction between hydrogen and nitric oxide at 700°C. 2 H2(g) + 2 NO(g) - 2 H20(g) + N2(g) Experiment [H2]/M [NO]/M Initial rate/M-s-1 0.012 0.031 4.5x10-6 0.0060 0.031 2.2x10-6 3 0.012 0.0155 1.1x10-6 (a) What is the rate law for the reaction? (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad Help Greek - (b) Calculate the rate constant for the reaction. 4.0 (c) Suggest a plausible reaction mechanism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate. Omit states-of-matter from your answer.) First step: chemPad Help Greek - Second step: chemPad Help Greek
Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1
For the reactionNO2 (g)+CO(g)NO(g)+CO2(g)calculate the order of the reaction with respect to the following reactants according to the following experimental data: Experiment [NO2]0(M) [CO]0(M) Initial Rate, –ΔΔ[NO2]/ΔΔt (M/s) 1 0.263 0.826 1.44 × 10–5 2 0.263 0.413 1.44 × 10–5 3 0.526 0.413 5.76 × 10–5 See Periodic Table Order of the reaction with respect to NO2: Order of the reaction with respect to CO:
The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.8e-4 1/s at 45°C. Let the inital concentration of N2O5 be 1.65e-2 mol/L. What is the half-life of the reaction? How long would it take for N2O5 to decrease to 1.00e-2 mol/L from its initial value? How long would it take for N2O5 to decrease to 75% of its inital value. Sketch [N2O5] versus time
A certain first order reaction has k = 2.51 s-1 . If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs
The rate constant for this second‑order reaction is 0.640 M−1⋅s−1 at 300 ∘C. A⟶products How long, in seconds, would it take for the concentration of A to decrease from 0.820 M to 0.220 M?
Nitesh
A synthetic surfactant (S) is known to decompose in aqueous solution according to the following reaction: S (aq)Products At 25.5°C, a 0.603 M solution of S was prepared and allowed to decompose. The reaction reached its first half life after 7 minutes. From the initiation of the reaction, the reaction reached its second half life after 10.5 minutes. Which of the following statements (i through vi) are true of the reaction at this temperature? I. The duration of the 3rd half life will be 10.5 minutes ii. The 3rd half life will be reached 12.25 minutes after the initiation of the reaction iii. The duration of the 3rd half life will be 3.5 minutes iv. Doubling the concentration of A will double the initial rate of reaction v. Doubling the concentration of A will quadruple the initial rate of reaction vi. Doubling the concentration of A will have no effect on the initial rate of reaction
The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
A student obtained the following data for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H₂(g) 9.40x10-2 [PH3], M time, s 0 4.70x10-2 29.9 2.35x10-2 1.18x10-2 89.7 59.8 (1) What is the half-life for the reaction starting at t = 0 s? What is the half-life for the reaction starting at t = 29.9 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? (3) Based on these data, what is the rate constant for the reaction?
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