For the reaction 2NO(g) + O₂(g) + 2NO₂(g) the following data were collected for the rate of disappearance of NO in the reaction Experiment [NO (M) (O₂) (M) Initial Rate (M/s) 00120 1.41 x 102 00125 00250 0 0252 1.13 x 101 0.0252 00125 5.64 x 10-2 1 2 3 What is the average value of the rate constant for the disappearance of NO calculated from the three data sets? Express the rate constant in the provided units to three significant figures. View Available Hint(s) Submit Part D VAX |A|NO| AL Request Answer ? What is the rate of disappearance of NO when [NO] -0.0800 M and (O₂)-0.0199 Af? Express the rate in molarity per second to three significant figures. View Available Hint(s) ΑΣΦΑ 4 M-21 ? M/s

For the reaction 2NO(g) + O₂(g) + 2NO₂(g) the following data were collected for the rate of disappearance of NO in the reaction Experiment [NO (M) (O₂) (M) Initial Rate (M/s) 00120 1.41 x 102 00125 00250 0 0252 1.13 x 101 0.0252 00125 5.64 x 10-2 1 2 3 What is the average value of the rate constant for the disappearance of NO calculated from the three data sets? Express the rate constant in the provided units to three significant figures. View Available Hint(s) Submit Part D VAX |A|NO| AL Request Answer ? What is the rate of disappearance of NO when [NO] -0.0800 M and (O₂)-0.0199 Af? Express the rate in molarity per second to three significant figures. View Available Hint(s) ΑΣΦΑ 4 M-21 ? M/s

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

The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and I2(g) is given here. What is the activation energy for the reaction? 2HI(g) ⟶ H2(g) + I2(g)
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
The balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
The data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
Using the data in the table, determine the rate constant of the Trial [A] (M) [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.210 0.0157 A + 2B C+D 0.220 0.420 0.0157 3 0.440 0.210 0.0628 Units k = M-ls-1 M-2s-1 M-s-1
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) | Rate (M/s) reaction and select the appropriate units. 0.250 0.260 0.0234 A + 2B → C + D 0.250 0.520 0.0234 3 0.500 0.260 0.0936 Units k = M.s-1 M-²s¬1 M-ls-1
X2 + Y₂ → 2Z R = k[Y₂] Trial [X₂]. (M) [Y₂], (M) Initial Rate (M/hr) 1 0.100 0.100 2.15 x 10-3 2 0.100 0.300 6.45 x 10-3 3 0.300 0.200 4.30 x 10-³ What is the rate constant for the reaction given the rate law and data? k = [?] Enter the answer choice number. Rate Law Expression Enter
Given the following data, determine the rate law for the reaction 2 NO(g) + O2g)22 NO2(g) Experiment [NO] (M) [O2] (M) Rate (M/s) 1 0.0300 0.0200 3.6 x 10-4 2 . 0.0600 0.0200 7.2 x 10-4 3 0.0600 0.0400 14.4 x 10-4 a) Determine the order of the reaction for each reactant, N, and 02. b) Write the rate law rate equation. ' ) ) Determine the value of the rate constant. (
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
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