You and a coworker have developed a molecule that has shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law: rate = k[AV]' [V]' You have been given the following data from your coworker: [V], = 0.30 M [AV], = 1.0 × 10-4 M A plot of In[AV] versus t(s) gives a straight line with a slope of -0.41 s¬1. What is the value of the rate constant k for this reaction? Rate constant = L. mol-1.s-1

You and a coworker have developed a molecule that has shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate law: rate = k[AV]' [V]' You have been given the following data from your coworker: [V], = 0.30 M [AV], = 1.0 × 10-4 M A plot of In[AV] versus t(s) gives a straight line with a slope of -0.41 s¬1. What is the value of the rate constant k for this reaction? Rate constant = L. mol-1.s-1

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 reaction in aqueous acidic solution occurs as shown by the balanced chemical equation below: H2O2(aq) + 3 I (aq) + 2 H* (aq) 13 (aq) + 2 H20(I) In the first 40.0 seconds of the reaction, the concentration of I' changes from 1.000 M to 0.868 M. Use the information to determine the average rate of the reaction within the first 40.0 seconds of the reaction. O 3.20x103 M/s O 1.10x10-3 M/s O 4.40x10-3 M/s O 2.20x10-3 M/s
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
The data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =
Consider this reaction: NH,ОH (аq) — NH; (aq)+н,0(ад) 4 At a certain temperature it obeys this rate law. rate = (0.071 Ms")[NH,OH Suppose a vessel contains NH OH at a concentration of 0.410M. Calculate how long it takes for the concentration of NH,OH to decrease to 7.0% of its 4 initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
A reaction has a rate law of Rate = (1.25 M⁻²s⁻¹)[A][B]². What concentration of [B] would give the reaction a rate of 0.0455 if the concentration of [A] is 0.250 M?
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
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:
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
The rate of a certain reaction is given by the following rate law: rate = k[N,][H] Use this information to answer the questions below.
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
Consider the reaction described by the equation С,Н, Вr, (aq) + 3Г (аq) — С,н,(8) + 2 Br (aq) + I5 (aq) The rate law is rate = k[C,H,Br,][I¯] where k = 0.00594 M-1. s-!. What are the missing entries in the table? Run [C,H,Br, lo (M) [I-], (M) Initial rate of formation of C,H, (M-s -) 1 0.245 0.00143 0.245 y 0.000713 3 0.245 0.245
Consider the experimental data collected for the following chemical reaction: 2H2(g) + 2NO(g) → N2(g) + 2H2O(g) Trial Initial [H2] (mol/L) Initial [NO] (mol/L) Rate of Reaction (mol/L∙s) 1 0.031 0.0025 2.0 x 10-3 2 0.062 0.0025 4.0 x 10-3 3 0.031 0.0050 8.0 x 10-3 4 0.062 0.0050 1.6 x 10-2 Which action will have more effect on the rate of this reaction; changing the concentration of H2(g) or that of NO(g)? Explain your reasoning by considering the orders of reactants and writing the corresponding rate law equation.