In a reaction A+ 2B-> C + D, initial rates weremeasured as shown inthe reaction with [A]O = 0.200 M and [B]0 = 0.400 M?(A) 3.20 \times 10-5 M s-1(B) 4.00 \times 10-5 M s-1(C) 5.00 \times 10-5 M s-1(D) It cannot be determined from the information given

To analyze the reaction and determine the rate law, we need more information about the initial rates…

Answered: In a reaction A+ 2B-> C + D, initial…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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In 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?
The scenes depict four initial reaction mixtures for thereaction of A (blue) and B (yellow), with and without a solidpresent (gray cubes). The initial rate, -Δ[A]/Δt(in mol/L s),is shown for each sphere representing 0.010 mol and the con-tainer volume at 0.50 L.(a) What is the rate law in the absence of a catalyst?(b) What is the overall reaction order?(c) Find the rate constant.(d) Do the gray cubes have a catalytic effect? Explain.
If the rate law for the reaction A ⟶Products is rate = k[A]2 , calculate the value of k from the following data: [A] (M) Initial Rate (M/s) 0.40 0.240 (A)0.15 M-1s-1 (B)0.015 M-1s-1 (C)0.00015 M-1s-1 (D)1.5 M-1s-1
What is the order of the reaction with respects to B and why is that? Please explain .
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
Consider the following balanced chemical equation: H2O2 (aq) + 3 r (aq) + 2 H (aq) >l (aq) + 2 H,O (I) If the concentration of iodide (la) decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s
What amount of time is required for the concentration of A to decrease from 0.800 M to 0.180 M in the zero- order reaction A->B? (k = 0.0567 M*s1)
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)
In 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?

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In a reaction A+ 2B-> C + D, initial rates were measured as shown in the reaction with [A]O = 0.200 M and [B]0 = 0.400 M ? (A) 3.20 \times 10-5 M s-1 (B) 4.00 \times 10-5 M s-1 (C) 5.00 \times 10-5 M s-1 (D) It cannot be determined from the information given