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
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…
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?
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.
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
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
Given the rate law: Rate = k[NO2]2[Cl2] By what factor does the rate change if each of the following changes occurs? Factor (enteras decimal, if <1) (a)[NO2] is tripled (b) [NO2] and [Cl2] are doubled (c)[Cl2] is halved
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
Given the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT). (A) DH = +45 kJ/mol; Ea = 75 kJ/mol; (B) DH = +35 kJ/mol; Ea = 65 kJ/mol; (C) DH = -35 kJ/mol; Ea = 75 kJ/mol; (D) DH = -45 kJ/mol; Ea = 65 kJ/mol;
The isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the equations above. Here C3H6* is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure?
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?