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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.2: Effect Of Concentration On Reaction Rate
Problem 11.4E
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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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