Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: elementary reaction NO (g) + Br₂ (g) → NOBr₂ (g) 2 NOBr₂ (g) +NO (g) → 2NOBr (g) step 1 k₁ k₂ Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate constant rate = k

Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: elementary reaction NO (g) + Br₂ (g) → NOBr₂ (g) 2 NOBr₂ (g) +NO (g) → 2NOBr (g) step 1 k₁ k₂ Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate constant rate = k

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

A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂ (g) + O₂ O₂(g) She fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time [SO3] (seconds) 0 0.800M 0.10 0.384M 0.20 0.252M 0.30 0.188M 0.40 0.150M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 ☐•☐ × Ś ? allo Ar 8 K
Consider the reaction: A + B → The following rate law was experimentally determined: rate = If the concentration of both A and B double, the rate will products k[A][B]? quadruple. increase by a factor of sixteen. double. increase by a factor of eight. triple.
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O₂(g) → 2 NO2(g) [0₂] (M) [NO] (M) Rate (M s-¹) 0.0100 0.0150 0.0150 0.0100 0.0100 0.0200 10.0 22.5 45.0 J What is the rate law for this reaction under these conditions? Rate = k [0₂]2 [NO]² Rate = k [0₂] [NO]² Rate = k [0₂]²2 [NO] Rate = k [0₂] [NO] G
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.81M 0.376M 105 M/s 1.81M 0.0561 M 1.19 × 105 M/S 0.236M 0.376M 1.36 × 104 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 = k0.0² 0 8.00 × k = x10 0.0 X
Some measurements of the initial rate of a certain reaction are given in the table below. [N] N2 H, initial rate of reaction 1.89M |0.180M 0.848 M/s 1.89М |0.686M 12.3 M/s 0.689M| 0.180M 0.113 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 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| х10 k =
Direction:Express the rate of the following chemical reactions in terms of the change in concentration of the reactants or products. 1.2NO2(g)→N2 (g)+ 202 (g) 2.N2 (g)+ 3H2 (g)→2NH3 (g) 3.2C4H10 (g)+ 1302 (g)→8CO2 (g)+ 10H2O(g)
For the decomposition of gaseous dinitrogen pentoxide, 2N2O5(g) → 4NO2(g) + O2(g) the rate constant is k = 2.8 × 10-3 s-1 at 60°C. The initial concentration of N2Os is 2.95 mol/L in a closed container at 60°C. After 3.75 min of reaction, what will be the mole fraction of NO2 in the gaseous mixture?
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) She fills a reaction vessel with Cl₂O5 and measures its concentration as the reaction proceeds: time (minutes) 0 10. [CI,Os] 0.300M 0.161M 20. 0.0864M 30. 0.0464M 40. 0.0249M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = x10 0.0 X 5
3. Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25 °C. If a 1.5-L reaction vessel initially contains 745 torr of N2O5 at 25 °C, what partial pressure of O2 is present in the vessel after 215 minutes?
The reaction A(aq) + B(aq) → Products(aq) was studied, and the following data were obtained: 0.28 0.14 [A]o (mol/L) 0.070 0.56 0.42 0.28 0.21 0.21 [B]o (mol/L) The rate constant for the reaction without units is Initial rate (mol/Los) 1.23x10-1 4.12×10-2 1.54x10-2 1.23x10-1
Find the intial rate of disappearance of Br2 when NO =.329 and BR2 =.181
Cyclobutane, C4H8, consisting of molecules in which four carbon atoms for a ring, decomposes when heated to give ethylene. C4H8(g) → 2C2H4(g) The reaction is first order. In an experiment, the initial concentration of cyclobutane was (3.500x10^-3) M. After heating at 450 °C, for (5.55x10^2) s, this was reduced to (2.6090x10^-3) M. What was the concentration of cyclobutane after a total of (1.008x10^3) s? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.