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...

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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
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Write rate law for the chemical reaction ?
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.
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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.
E. For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A][A](MM) [B][B](MM) [C][C](MM) Initial rate(M/sM/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
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?
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
Suppose you are studying the kinetics of the reaction between the peroxydisulfate ion and iodide ion. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [S2O82–] (M) [I–] (M) Initial Rate (M/s) 1 0.27 0.38 2.05 2 0.40 0.38 3.06 3 0.40 0.22 1.76 Based on the data, choose the correct exponents to complete the rate law. rate=k[S2O82–]a[I–]b a= b=
Suppose you are studying the kinetics of the reaction between the peroxydisulfate ion and iodide ion. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [S2O82–] (M) [I–] (M) Initial Rate (M/s) 1 0.27 0.38 2.05 2 0.40 0.38 3.06 3 0.40 0.22 1.76 Based on the data, choose the correct exponents to complete the rate law. rate=k[S2O82–]a[I–]b a= b=