For the following general reaction, rate = k[A] and k = 1.3 x 10 -Ms A+B - 20 Use this information to fill in the missing table entries. Experiment [A] (M) B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 x 106 2 0.026 0.250 3 0.500 2.20 x 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M

For the following general reaction, rate = k[A] and k = 1.3 x 10 -Ms A+B - 20 Use this information to fill in the missing table entries. Experiment [A] (M) B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 x 106 2 0.026 0.250 3 0.500 2.20 x 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M

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

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.
Consider the following reaction and information: A + 2B → 3C rate = k{B} Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?
2. For the following reaction at 500 °C Cl2 (g) + H2 (g) 2 HCI (g) + the following data were collected: Experiment [H2 ] [ Cl2 ] Initial Reaction Rate 1 0.025 M 0.012 M 1.60 x 10 4 2 0.050 M 0.012 M 6.40 x 10 -4 3 0.050 M 0.048 M 6.40 x 10 -4 Give a rate law expression for this reaction and also calculate the value of the rate constant (k) for this reaction. What is the overall order of this reaction?
please answer both please i will upvote ( if you have plan to answer only one then please skip , let someone accept the question who can do both )
Given this data in a study on how the rate of a reaction was affected by the concentration of the reactants (Show work on separate page for the rest of the exam and submit in assignments) run [A] [B] [C] rate, M/hr 1 0.200 0.100 0.600 5.0 2 0.200 0.400 0.400 80.0 3 0.600 0.100 0.200 15.0 4 0.200 0.100 0.200 5.0 5 0.200 0.200 0.400 20.0 a) Give the rate law. b) Give the rate constant.
Attem Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.300 0.400 0.0112 2 0.300 0.800 0.0112 A + 2B C+D 3 0.600 0.400 0.0448 Units k =|| %D TOOLS M-'s-1 x10 |help terms of use contact us careers privacy policy about us prime video W
1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4² Given a graph of moles S₂Og 2 consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction? 2. The initial rates listed in the following table were determined for the reaction: H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1) Trial Initial [H₂PO3¯], (M) Initial [OH], (M) Initial Rate of Consumption (M/s) 1 0.025 0.030 0.432 2 0.100 0.030 1.728 3 0.100 0.015 0.864 a) What is the rate law? b) What is the value of the rate constant, k? c) What is the initial rate when the initial concentrations of both reactants are 0.12 M? 3. The following experimental data was obtained for the bromination of acetone at 30°C. 21 +2 H+H2O2 → I2 + 2 H₂O Trial Initial [I] (M) Initial [H+] Initial [H2O2] (M) Rate (M/sec) (M) 1 0.001 0.005 0.001 2.0 x 104 2 0.002 0.005 0.001 4.0 x 10+ 3 0.006 0.002 0.001…
Be sure to answer all parts. For the following general reaction, rate = k[A]2 and k=1.3 × 10 2 M¹g¹; A+B 2C Use this information to fill in the missing table entries. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 × 10-6 2 0.026 0.250 3 0.500 2.20 × 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M
6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
just need standard error for K
A: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate of Zn2+ formation if its concentration rises from 0.00 to 0.069 M in 2 minutes and 12 seconds? Group of answer choices 0.031 M/s 2.1 x 10-3 M/s 1.3 x 10-4 M/s 5.2 x 10-4 M/s B: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1