**write out your work for this problem on your work upload sheet.* Consider the following hypothetical reaction mechanism for the oxidation of bromotrifluoromethane, a halon, by OH in the atmosphere, where each step is an elementary reaction step. OH (g) +CBRF3 (g) HOB (g) + CF3 (g)OH(g)+ CBrF,(g) HOBr(g) + CF;(g) - → CF (g) + 0OH (g) OH (9) + OCF3 (9)CF,(g)+ OOH(g) → OH(8) + OCF,(g) OCF (g) + NO (g) → COF2 (g) + FNO (9)OCF;(g) + NO(g) → COF ,(g) + FNO(g) | Write the overall reaction, and identify any catalysts or intermediate(s) that take part in the process. You can also write the overall reaction for your Gradescope upload if you think that is easier. You do need to include any catalyst or intermediates here. If none, write "none". If there is more than one species, you can separate them with commas. You do not need to include the states, and don't worry about subscripts. For example, NO2 would be written as NO2. Overall reaction: Catalyst(s): Intermediate(s):

**write out your work for this problem on your work upload sheet.* Consider the following hypothetical reaction mechanism for the oxidation of bromotrifluoromethane, a halon, by OH in the atmosphere, where each step is an elementary reaction step. OH (g) +CBRF3 (g) HOB (g) + CF3 (g)OH(g)+ CBrF,(g) HOBr(g) + CF;(g) - → CF (g) + 0OH (g) OH (9) + OCF3 (9)CF,(g)+ OOH(g) → OH(8) + OCF,(g) OCF (g) + NO (g) → COF2 (g) + FNO (9)OCF;(g) + NO(g) → COF ,(g) + FNO(g) | Write the overall reaction, and identify any catalysts or intermediate(s) that take part in the process. You can also write the overall reaction for your Gradescope upload if you think that is easier. You do need to include any catalyst or intermediates here. If none, write "none". If there is more than one species, you can separate them with commas. You do not need to include the states, and don't worry about subscripts. For example, NO2 would be written as NO2. Overall reaction: Catalyst(s): Intermediate(s):

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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The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
The reduction of NO to N, with H,; 2NO(g) + 2H2(g) = N2(g) + 2H,0(g), is found to have the following experimentally determined rate equation: Rate =k[NO]²[H,] If the concentration of NO and H, were doubled then the rate of the reaction would: Decrease four fold Increase four fold Increase two fold Increase eight fold
rate constant 1 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂(g) + H₂O(g) 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. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, K₂, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. step elementary reaction t k = A 00 X
The formation of nitrosyl chloride is described by the following chemical equation: 2NO (g) + Cl₂ (g) → 2NOCI (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) +Cl₂ (g) NOCI₂ (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism. 11 × Ś
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E72.0 kJ/mol. If the rate constant of this -1 -1 reaction is 3.4 × 10² M² S at 308.0 °C, what will the rate constant be at 218.0 °C? Round your answer to 2 significant digits. - 1 - 1 k x10 X ? = M • S Ś
(a) In the reaction mechanisms given, there are some chemical species which will get produced in one step and get consumed in the other step and that are not in reactants nor in products of the total reaction. Such species are known as intermediates of a reaction as the name suggests. Therefore, in mechanism 1, the intermediates are (CH3)2CHOH2+, Cl-, (CH3)2CH+. and in mechanism 2: (CH3)2CHOH2+, Cl-. These ions are neither reactants nor products of the given total equation.
Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O S
Consider the hypothetical reaction A +B+ 2C → 2D + 3E where the rate law is ΔΙΑ = k[A][B]? At Rate An experiment is carried out where [A]o = 1.0 x 10-² M, [B]o 6.0 M, 2 and [C, = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mol -1 S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 19.0 seconds. Concentration M d. Calculate the concentration of C after 19 seconds. Concentration = M
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0094 M·s: 2 NH3 (g) → N2 (g)+3 H, (g) Suppose a 450. mL flask is charged under these conditions with 400. mmol Of ammonia. After how much time is there only 200. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
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The differential rate laws for the balanced chemical reaction: aA(aq) + bB (aq) + CC (aq) → product is given by: raterxn = k [A]³[C]³ [B]³ What are the order in each chemical, as well as the overall order of the chemical kinetics? Place your answer in each box, respectively! Provide detailed solution (The order of kinetics in A) = (The order of kinetics in B) = (The order of kinetics in C) = (The overall order of kinetics) =