A student obtained the following data for the decomposition of nitrosyl bromide at 10 °C. NOBr(g) →→→NO(g) + ½ Br₂(g) [NOBr], M seconds 7.74x10-² 0 3.87x10-2 21.9 (1) What is the half-life for the reaction starting at t=0 s? 21.9 Submit Answer What is the half-life for the reaction starting at t=21.9 s? 65.5 (2) Is the reaction zero, first, or second order? second ✓ 1.94x10-² 65.5 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Try Another Version S Does the half-life increase, decrease or remain constant as the reaction proceeds? increase (3) Based on these data, what is the rate constant for the reaction? .59 S 9.70x10-3 1 item attempt remaining 153 M-¹S-1 > Previous Next

A student obtained the following data for the decomposition of nitrosyl bromide at 10 °C. NOBr(g) →→→NO(g) + ½ Br₂(g) [NOBr], M seconds 7.74x10-² 0 3.87x10-2 21.9 (1) What is the half-life for the reaction starting at t=0 s? 21.9 Submit Answer What is the half-life for the reaction starting at t=21.9 s? 65.5 (2) Is the reaction zero, first, or second order? second ✓ 1.94x10-² 65.5 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Try Another Version S Does the half-life increase, decrease or remain constant as the reaction proceeds? increase (3) Based on these data, what is the rate constant for the reaction? .59 S 9.70x10-3 1 item attempt remaining 153 M-¹S-1 > Previous Next

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

View Policies Show Attempt History Current Attempt in Progress X Incorrect. -1 The catalyzed decomposition of ethanol at 327°C has a rate constant of 4,00 x 105 L mol¹1A graph of the reciprocal of ethanol concentration versus time gives a straight line. The chemical equation for the reaction at this temperature is C₂H₂OH(g)-CHg) + H₂O(g) If the initial concentration of ethanol is 0.023 mol L¹, how long will it take for the pressure to reach 1.4 atm at 327°C? i 60 eTextbook and Media Hint 1. The unit of the rate constant indicates the order of reaction. 2. Use partial pressures and the universal gas law to calculate moles and concentrations. 3. Set up a table showing initial molar concentrations and concentrations at time t Save for Later 45 hours 80 d F4 MacBook Air F6 Attempts: 4 of 15 used Submit Answer Assistance Used 8: DII 8² St
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 following is the experimental data for the rate of reaction: Q (g) + 2T (g) --> T2Q (g) in some conditions Experiment [Q](M) [T](M) V (M/second) 1 0,1 0,1 0,0125 2 0,2 0,1 0,05 3 0,1 0,2 0,1 if [Q] and [T] are changed to 0.5M each, then the reaction rate (v) at that time is?
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?
Answer in minutes
The following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: NO, (aq) +O,(g) NO, (aq) +0,(g) > Experiment [NO2 lo (M) [O3lo (M) Initial Rate (M/s) 1 0.0100 0.0050 25.0 0.0150 0.0050 37.5 3 0.0200 0.0050 50.0 0.0200 0.0200 200.0
14. The data in the table below was collected for the following reaction at 425°C. 2 A(g) + 3 B(g) →3 C(g) +2 D(g) Trial 1 2 3 4 [A] i, M [B]i, M Initial Rate, M/s 0.100 0.050 1.0 × 10-3 0.050 0.050 2.5 × 10-4 0.100 0.100 2.0 × 10-3 0.150 0.100 4.5 x 10-3 a. What is the rate law for this reaction? b. What is the overall order of the reaction? 15. The rate constant for the following reaction is 3.00 x 10-3 M-1 min-1 at 500 K:
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.
1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth
The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1
3) The reaction 2NO(g) + O2(g) → 2 NO₂(g) was studied, and the following data were obtained where Δ[02] At Rate = [NO]. [0₂]0 (molecules/cm³) (molecules/cm³) 1.00 x 1018 3.00 x 10¹8 2.50 × 1018 1.00 x 1018 1.00 × 10¹8 2.50 × 1018 Submit Answer Initial Rate (molecules/cm³.s) 2.00 × 1016 1.80 x 10¹7 3.13 x 10¹7 What would be the initial rate for an experiment where [NO], = 1.57 x 10¹8 molecules/cm³ and [0₂]0 = 8.82 x 10¹8 molecules/cm³? 3 Rate = molecules/cm³.s Try Another Version [References] 5 item attempts remaining Show Hint
A) How long will it take for the concentration of A to decrease from 1.400 M to 0.295 for the zero order reaction A → Products? (k = 0.0345 M/s) B) The half-life for the second order reaction A → Products is 4.57 min. What is the value of the rate constant for the reaction if the initial concentration of A is 0.215?