Ethyl chloride, CH3 CH₂ Cl, used to produce tetraethyllead gasoline additive, decomposes, when heated, to give ethylene and hydrogen chloride. CH3 CH₂Cl(g) → C₂H4 (9) + HCl(g) The reaction is first order. In an experiment, the initial concentration of ethyl chloride was 1.00 x 107 M. After heating at 500°C for 155 s, this was reduced to 6.70 x 10-4 M. What was the concentration of ethyl chloride after a total of 247 s? Concentration = M

Ethyl chloride, CH3 CH₂ Cl, used to produce tetraethyllead gasoline additive, decomposes, when heated, to give ethylene and hydrogen chloride. CH3 CH₂Cl(g) → C₂H4 (9) + HCl(g) The reaction is first order. In an experiment, the initial concentration of ethyl chloride was 1.00 x 107 M. After heating at 500°C for 155 s, this was reduced to 6.70 x 10-4 M. What was the concentration of ethyl chloride after a total of 247 s? Concentration = M

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 rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=39.0 kJ/mol. If the rate constant of this -1 reaction is 6.0 x 102 M's -1 at 9.0 °C, what will the rate constant be at 53.0 °C? Round your answer to 2 significant digits. -1 k = x10
Consider the following reaction: A + B --> products. The rate law was found to be rate = k[A][B]^2. If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the equation? How will this affect the time required for the reaction to reach completion?
A zero order reaction has a constant rate of 3.1 × 10−4 mol·L−1·s−1. If after 60 seconds the concentration has dropped to 4.7 × 10−2 mol·L−1, what was the initial concentration (in mol·L−1)? Express your answer to two significant figures.
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] Rate = k [NO₂(g)]² [03(g)] Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] (b) If the rate constant for this reaction at a certain temperature is 97900, what is the reaction rate when [NO₂(g)] = 0.587 M and [03(9)] = 1.40 M? Rate = 2 NO₂(g) + 03(9) → N₂O5(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.17 M while the concentration of O3(g) is 1.40 M? M/S
Consider the hypothetical reaction: A + B + 2C → 2D + E where the rate law is Rate = -ALA) = k[A][B]2 An experiment is carried out where [Alo = 7.200 x 102 M, [B]. = 2.500 M and [Cla = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M2s1. Answer:
2
Aluminum will slowly react with oxygen to produce aluminum oxide. The rate of this reaction has been measured for two different reaction conditions. The rate is 4 mmol/s when 2 M Al is reacted with 3 M O, and the rate is 2 mmol/s when 1 M Al is reacted with 3 M O. What would be the value of M for the rate equation, rate = k [Al]^m[O}^n
Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cl, (g) · SO2(g) + Cl, (g)
The rate of a certain reaction is given by the following rate law: rate=k|N, || H2 K[N][H° Use this information to answer the questions below. What is the reaction order in N,? 1 х10 What is the reaction order in H2? ? 2 What is overall reaction order? 3 At a certain concentration of N, and H2, the initial rate of M reaction is 5.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 0.640 M/ s when [N2] - 2 • S 1.8 M and [H2] 1.4 M. Calculate the value of the rate - 1 k = |M constant. Round your answer to 2 significant digits.
Consider the reaction, 2A + B → C. If the rate law for this reaction is rate = k{A}²{B}, what is true of this reaction? It is an elementary reaction. C is an intermediate. B is an intermediate. The rate is second order overall.