The following reaction is investigated to determine its rate law: 2NO(3) + 2H2(3) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-1) INO) 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10-8 0.80 x 10-4 0.60 x 10-4 8.0 x 10-8 What is the rate law for the reaction? O rate = k [NO][H2] O rate = k [NO]?[H2]? O rate = k [NO][H21² O rate = k [NO]?[H2] What is the value of the rate constant? k= i x 105 O L2 mol-2 s-1 O s-1 O mol L-s-1 O L° mol-3 s-1 O L mol-1s-1
The following reaction is investigated to determine its rate law: 2NO(3) + 2H2(3) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-1) INO) 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10-8 0.80 x 10-4 0.60 x 10-4 8.0 x 10-8 What is the rate law for the reaction? O rate = k [NO][H2] O rate = k [NO]?[H2]? O rate = k [NO][H21² O rate = k [NO]?[H2] What is the value of the rate constant? k= i x 105 O L2 mol-2 s-1 O s-1 O mol L-s-1 O L° mol-3 s-1 O L mol-1s-1
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.51QP: In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were...
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![The following reaction is investigated to determine its rate law:
2NO(3) + 2H2(3) → N2{g) + 2H2O(g)
Experiments yielded the following results:
Initial Concentrations (mol L-1)
Initial Rate of Formation of N2
(mol L-Is-1)
INO)
[H,]
0.40 x 10-4
0.30 x 10-4
1.0 x 10-8
0.80 x 10-4
0.30 x 10-4
4.0 x 10-8
0.80 x 10-4
0.60 x 10-4
8.0 x 10-8
What is the rate law for the reaction?
O rate = k [NO][H2]
O rate = k [NO]?(H,]?
O rate = k [NO][H2]²
O rate = k [NO]?[H2]
What is the value of the rate constant?
k = i
x 105
O L2 mol-2 s-1
s-1
mol L-15-1
O L³ mol-3s-1
O L mol-1s-1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fddee7e9a-8e52-47fe-9b74-c5d35111042c%2F37f35f40-fdef-405c-b37a-27445191e757%2F2d66j8_processed.png&w=3840&q=75)
Transcribed Image Text:The following reaction is investigated to determine its rate law:
2NO(3) + 2H2(3) → N2{g) + 2H2O(g)
Experiments yielded the following results:
Initial Concentrations (mol L-1)
Initial Rate of Formation of N2
(mol L-Is-1)
INO)
[H,]
0.40 x 10-4
0.30 x 10-4
1.0 x 10-8
0.80 x 10-4
0.30 x 10-4
4.0 x 10-8
0.80 x 10-4
0.60 x 10-4
8.0 x 10-8
What is the rate law for the reaction?
O rate = k [NO][H2]
O rate = k [NO]?(H,]?
O rate = k [NO][H2]²
O rate = k [NO]?[H2]
What is the value of the rate constant?
k = i
x 105
O L2 mol-2 s-1
s-1
mol L-15-1
O L³ mol-3s-1
O L mol-1s-1
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