Describe the overall reaction order for the chemical reaction with rate law v = k[A][B]?[C]³ when. B is in great excess pseudo second order A is in great excess pseudo zero order Cis in great excess pseudo third order pseudo fifth order pseudo first order pseudo fourth order

Describe the overall reaction order for the chemical reaction with rate law v = k[A][B]?[C]³ when. B is in great excess pseudo second order A is in great excess pseudo zero order Cis in great excess pseudo third order pseudo fifth order pseudo first order pseudo fourth order

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

Consider the reaction described by the equation С,Н, Br, (aq) + 31 (аq) — C,H,(g) + 2 Br¯(aq) + I, (aq) 4 The rate law is rate = k[C,H,Br, ][I¯] where k = 0.00483 M-1. s-1. What are the missing entries in the table? Run [C,H,Br, lo (M) | [I¯]o (M) Initial rate of formation of C,H, (M-s ) 4 1 0.299 0.00173 2 0.299 y 0.000864 3 0.299 0.299
For the following reaction 2A > A2 This is a zero rate order. The rate constant is y = -0.0034x +0.9996 What is the rate law expression? What is the concentration at 290 seconds? Time [A](M ) 0 1 25 0.914 50 0.829 75 0.744
4. Consider three hypothetical reactions of the type A → products. One of the reactions is zeroth order, one is first order, and one is second order. If they all have the same numerical value of the rate constant k (in units of M s ¹, s and M¹s¹, -1 -1 9 respectively), what must be the initial concentration [A]o if the half-lives are equal for a) the zeroth- and first-order reactions, b) the zeroth- and second-order reactions, and c) the first- and second-order reactions.
24
The rate constant for the second order reaction 2 NO2 - 2 NO + O2 is 0.24 M's. If a 1.38 M sample of NO2 reacts for 47.7 seconds, what concentration of NO2 wil remain? Report your answer to two decimal places. |Al = - kt +|Alo InJAl = - kt + InlAlo TAI = kt + TAlo
Consider the reaction described by the equation C,H,Br, (aq) + 3 I (aq) C,H, (g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k[C,H¸Br,][I¯] where k = 0.00504 M-1. s-1. What are the missing entries in the table? Run [C,H,Br,h (M). [I¯], (M) Initial rate of formation of C,H, (M-s) 1 0.162 0.000529 0.162 y 0.000265 3 0.162 0.162 M X = M y = z = M-s-1
A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)
Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N20, and water. 2NO(g) + H2 (g) → N½O(g) + H20(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Initial Concentration of NO Initial Concentration of H2 Initial Rate of Reaction of NO Exp. 1 8.6 x 10-3 M 4.1 x 10-3 M 8.7 x 10-5 M/s 3 Exp. 2 1.7 x 10-2 M 4.1 x 10- M 3.5 x 10-4 M/s Exp. 3 8.6 x 10-3 M 8.2 x 10-3 M -4 1.7 x 10 M/s
A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=