2H, (g) + 2NO(g) = 2H,0(g) + N,(g) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2lo (M) [NO]o (M) Initial Rate (M/s) 1 0.212 0.136. 0.0267 2 0.212 0.272 0.0537 3 0.424 0.544 0.423 4 0.848 0.544 1.70 1st attempt Part 1 (1 point) Feedback Choose the correct rate law for the reaction at 1500°C. Choose one: O A. rate=k =k[H_][NO] 4 VIEW SOLUT 9 OF 11 QUESTIONS COMPLETED < 11/11 > A Atomic emission..pdf Determination of...pdf Chem.pdf (1).pdf

2H, (g) + 2NO(g) = 2H,0(g) + N,(g) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2lo (M) [NO]o (M) Initial Rate (M/s) 1 0.212 0.136. 0.0267 2 0.212 0.272 0.0537 3 0.424 0.544 0.423 4 0.848 0.544 1.70 1st attempt Part 1 (1 point) Feedback Choose the correct rate law for the reaction at 1500°C. Choose one: O A. rate=k =k[H_][NO] 4 VIEW SOLUT 9 OF 11 QUESTIONS COMPLETED < 11/11 > A Atomic emission..pdf Determination of...pdf Chem.pdf (1).pdf

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

5
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.
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.
Which one of the following is not a valid expression for the rate of the reaction below? 4NH3 + 702 → 4NO2 + 6H2O 1 A[02] At Ο1 ΔΙΝO] 4 At O 1 A[H2O] At O All of the above are valid expressions of the reaction rate. 1 A[NH3] 4 At hp Nengl Tov 732006020610 12 米 144 $ 4. 8
PLEASE ANSWER EVERYTHING ON THE PICTURES, THANK YOU
Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, (g) The initial reaction rates of four mixtures of H, and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 0.212 0.136 0.0393 2 0.212 0.272 0.0789 0.424 0.544 0.624 0.848 0.544 2.50 4.
Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234
I need your help please please
Hydrogen gas reduces NO to N2 in the following reaction:$$2H2(g)+2NO(g)2H2O(g)+N2(g)The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2]0 (M) [NO]0 (M) Initial Rate (M/s) 1 0.212 0.136 0.0333 2 0.212 0.272 0.0669 3 0.424 0.544 0.528 4 0.848 0.544 2.12 Determine the rate constant for the reaction at 1500°C.
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1
What is the rate for the zero order reaction A → Products when [A] = 0.200 M? (k = 3.57 M/min) M/min 1 2 3 C 7 8 9 +/- х 100 LO 4.