The overall reaction: 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g) was determined by thefollowing experimental data:ExperimentNOH2 (mol/L)Initial Rate of Reaction(mol/L)0.001(mol/(L-s))0.00210.0040.0020.0040.00830.0040.0010.00840.0040.0020.016a. Determine the rate law equation.b. Determine the rate constant, k.C. Calculate the expected reaction rate (in mol/L-s) when [NO] = 0.005 mol/Land [H2] = 0.005 mol/L.

Answer: Rate law for the given reaction is: r=k[NO]α[H2]β Here: r=rate of reactionk=rate constant α…

The overall reaction: 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g) was determined by the following experimental data: Experiment NO H2 (mol/L) Initial Rate of Reaction (mol/L) 0.001 (mol/(L-s)) 0.002 1 0.004 0.002 0.004 0.008 0.008 3 0.004 0.001 4 0.004 0.002 0.016 a. Determine the rate law equation. b. Determine the rate constant, k. C. Calculate the expected reaction rate (in mol/L-s) when [NO] = 0.005 mol/L and [H2] = 0.005 mol/L. %3!

The overall reaction: 2 NO (g) + 2 H2 (g) → N2 (g) + 2 H2O (g) was determined by the following experimental data: Experiment NO H2 (mol/L) Initial Rate of Reaction (mol/L) 0.001 (mol/(L-s)) 0.002 1 0.004 0.002 0.004 0.008 0.008 3 0.004 0.001 4 0.004 0.002 0.016 a. Determine the rate law equation. b. Determine the rate constant, k. C. Calculate the expected reaction rate (in mol/L-s) when [NO] = 0.005 mol/L and [H2] = 0.005 mol/L. %3!

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

Consider the plot that shows the concentration of the reactant A in the reaction A → B. Which expression would you use to find the average rate of the reaction between 10 and 20 seconds? 1.2 0.8 [A] 0.6 0.4 - 0.2 0- O 10 20 30 40 50 60 70 80 Time (s) O (0.75M-0.85M)/(20s-10s) -(0.75M-0.85M)/(20s-10s) -(0.85M-0.75M)/(20s-10s) O -(0.85M-0.75M)/(10s-20s) Concentration (M)
For the reaction: Bro3 (aq) + 5Br (aq) + 8H*(aq) → 3Br2(f) + H20(6) The initial rate of the reaction has been measured at the reactant concentrations show: Trial [BrO,] [H'] (mol/L) (mol/L) 0.10 [Br] (mol/L) Initial rate (mol/L-s) 1 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 0.10 0.10 0.20 32 The rate law expression will be: 234
2
Question 10 of 42 A reaction has the stoichiometry: 3A+B+C+D. The following data were obtained for the initial rate of formation of C at various concentrations of A and B. Initial Concentration [A] 0.10 0.20 0.20 [B] 0.10 0.20 0.10 Initial Rate of Formation of C (mol L-¹ s¹) Rate = K[A]²[B]⁰ Rate = K[A]²[B]² None of these. □ Rate = K[A]⁰[B]² Rate = K[A]¹[B]¹ 0.037 (a) What is the rate law for the reaction? eTextbook and Media 0.15 0.037 (b) What is the rate constant for the reaction? i Lmol-¹5-1 (c) What is the rate at which C is formed if [A] = 0.34 M and [B] = 0.78 M? i mol L-15-1
The chemical reaction between X and Y is known to be first order for each reactant. Find the unknown information in the table below.
Questions 1A 1B and 1C please
This question has multiple parts. Work all the parts to get the most points. The reaction 2NO(g) + Cl₂ (g) → 2NOCI(g) was studied at -10°C. The following results were obtained where A[C1₂] At Rate = [NO], [C12]o (mol/L) (mol/L) 0.12 0.12 0.12 0.24 0.24 0.24 Initial Rate (mol/L.min) 0.31 0.62 2.49 a What is the rate law? (Use k for the rate constant. ) Rate = k[NO]²[C1₂] b What is the value of the rate constant? Rate constant = L² mol². min
Try Again Your answer is incorrect. • Row 2: Your answer is incorrect. Please check your units. Some measurements of the initial rate of a certain reaction are given in the table below. N₂ H₂] initial rate of reaction 0.945 M 1.74M 1.00 × 106 M/s 0.945M 0.395M 5.15 × 10+ M/s 0.458M 1.74M 4.85 × 105 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k [N,][H, 5 k 3.5 X 10 - 2 - 1 M S x10 Ś
#2 please
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?
Thanking you for your help.....the question is attached
The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.