Consider the following hypothetical reaction: 2P + Q→ 2 R + S. The following mechanism is proposed for this reaction: P + P = T (fast) Q + T → R+ U (slow) U-R + S (fast) Substances T and U are unstable intermediates. What rate law is predicted by this mechanism? (a) Rate = k[P]? (b) Rate = k[P][Q] (c) Rate = k[P]°[QI (d) Rate = k[P][Q? (e) Rate = k[U]

Consider the following hypothetical reaction: 2P + Q→ 2 R + S. The following mechanism is proposed for this reaction: P + P = T (fast) Q + T → R+ U (slow) U-R + S (fast) Substances T and U are unstable intermediates. What rate law is predicted by this mechanism? (a) Rate = k[P]? (b) Rate = k[P][Q] (c) Rate = k[P]°[QI (d) Rate = k[P][Q? (e) Rate = k[U]

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 catalyzed decomposition of ethanol at 328°C has a rate constant of 4.00 x 105 L mol ¹s¹. A graph of the reciprocal of ethanol concentration versus time gives a straight line. The chemical equation for the reaction at this temperature is C₂H₂OH() C₂H.(g) + H₂O(g) If the initial concentration of ethanol is 0.022 mol L¹, how long will it take for the pressure to reach 1.4 atm at 328°C? hours
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) → O₂(g) + NO₂(g) The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 3.59 x 10° Ms at a certain temperature, calculate the initial reaction rate when [O,] and [NO] remain essentially constant at the values [0,10 = 5.61 x 10-6 M and [NO]o = 5.16 x 105 M, owing to continuous production from separate sources. initial reaction rate: 0.0009559 Incorrect Calculate the number of moles of NO₂(g) produced per hour per liter of air. Question Source McQuarrie Rock strik Unhares M
The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H20 → C;H1206 + CgH1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C,,H,,0,1] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are 22 isomers.) 1.8x10-11 Arrhenius equation at this temperature). (Enter unrounded values.) (a) In neutral solution, k at 26°C and 8.5x10-11 -1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s), and the rate constant (in s) for this equation at 48°C (assuming the kinetics remain consistent with the activation energy 108 kJ/mol frequency factor rate constant X s-1 (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10 M. How long (in s) will it take the solution to reach equilibrium…
The proposed mechanism for a reaction is (1) A(g)+ B(g) ⇌ X(g)[fast (2)X(g)+C(g) →Y(g)(slow)(3)Y(g) →D(g)(fast) (a) What is the overall equation?(b) Identify the intermediate(s), if any.(c) What are the molecularity and the rate law for each step?(d) Is the mechanism consistent with the actual rate law: rate k[A][B][C]?(e) Is the following one-step mechanism equally valid: A(g) +B(g) +C(g) → D(g)?
For the decomposition of gaseous dinitrogen pentaoxide,2N₂O₅(g) →4NO₂(g) +O₂(g), the rate constant is k=2.8X10⁻³ s⁻¹at 60°C. The initial concentration of N₂O₅ is1.58 mol/L. (a) What is [N₂O₅] after 5.00 min? (b) What frac-tion of the N₂O₅ has decomposed after 5.00 min?
The mechanism of a reaction occurs via two steps: Step 1: A + B → C + D Step 2: A + D → C Rate law for the reaction is Rate = [A] [B] (a) Determine rate determining step (slow step)? (b) Write the balance equation for the overall reaction. (c) Determine intermediate in the reaction.
Consider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.
The combustion of ammonia is shown below: 4NH:(g) + 50:(g) → 4NO(g) + 6H20(g) Write an equation that relates the rates of consumption of the reactants and the rates of formation of the products. At 298 °C, the rate of reaction (v) is 2.7 x 10 mol L-'s. Find the rate change of NH3, O2, NO and H20. (ii)
Consider the rate law: Rate = k [A]2[B][C]1/2. How does the rate of the reaction change if theconcentration of C is doubled? a) The rate increases by a factor of 1.414b) The rate increases by a factor of 1.732c) The rate reduces by a factor of 1.732d) The rate triplese) The rate reduces by a factor of 1.414
Determine Ea and A, the activation energy and pre-exponential factor. What is the value of the rate constant at 100(⁰C)?
Consider the following reaction: Q:4-1 2 NO(g) + 2 H;(g) → N;(8) + 2 H,0(g) (a) The rate law for this reaction is first order in H, and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 × 10ª M-²s¯!, what is the re- action rate when [NO] = 0.035 M and [H,] = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H, is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H,] is increased to 0.030 M? %3D
The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3