Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) (a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M? Rate = _______ M/s.
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g) (a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M? Rate = _______ M/s.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Consider the following reaction:
4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)
(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?
(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?
Rate = _______ M/s.
(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?
Rate = _______ M/s
(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?
(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?
Rate = _______ M/s.
(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?
Rate = _______ M/s
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