The reaction shown below has a rate constant (k) of 8.45x10-4 s-1. If the reactionbegins with AB at a concentration of 0.970 M, what will the AB concentration beafter 910.0 s?2 AB(g) → A2(g) + B2(g)0.56 M0.45 M0.20 M0.77 M Based on the rate law shown below, the reaction is third-order.k[A]² [B]rate||TrueFalseIf the half-life of a reaction gets longer as the initial concentration of the reactant isincreased, the reaction must be order.secondO firstzero

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The reaction shown below has a rate constant (k) of 8.45x10“ s-². If the reaction begins with AB at a concentration of 0.970 M, what will the AB concentration be after 910.0 s? 2 AB(g) A2(g) + B2(g) 0.56 M 0.45 M 0.20 M ) 0.77 M

The reaction shown below has a rate constant (k) of 8.45x10“ s-². If the reaction begins with AB at a concentration of 0.970 M, what will the AB concentration be after 910.0 s? 2 AB(g) A2(g) + B2(g) 0.56 M 0.45 M 0.20 M ) 0.77 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...

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Question

The reaction shown below has a rate constant (k) of 8.45x10-4 s-1. If the reaction
begins with AB at a concentration of 0.970 M, what will the AB concentration be
after 910.0 s?
2 AB(g) → A2(g) + B2(g)
0.56 M
0.45 M
0.20 M
0.77 M

Based on the rate law shown below, the reaction is third-order.
k[A]² [B]
rate
||
True
False
If the half-life of a reaction gets longer as the initial concentration of the reactant is
increased, the reaction must be order.
second
O first
zero

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