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The rate law for the reaction 2NO(g) + 2H₂(g) - N₂(g) + 2H₂O(g) is rate = k[NO]²[H₂] If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 × 10-6 mol L-1, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 9.56 S-1 mol L-¹5-1 L³ mol-³ s-1 L² mol-² s-1 L mol-¹ S-1

The rate law for the reaction 2NO(g) + 2H₂(g) - N₂(g) + 2H₂O(g) is rate = k[NO]²[H₂] If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 × 10-6 mol L-1, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 9.56 S-1 mol L-¹5-1 L³ mol-³ s-1 L² mol-² s-1 L mol-¹ S-1

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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The rate law for the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(g) is rate = K[NO]²[H₂] -1 If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 x 10-6 mol L-¹, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 X 9.56 5-1 mol L-¹5-1 L³ mol-³ s-1 3 L² mol-2 s-1 L mol-¹ S-1
Transcribed Image Text:The rate law for the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(g) is rate = K[NO]²[H₂] -1 If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 x 10-6 mol L-¹, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 X 9.56 5-1 mol L-¹5-1 L³ mol-³ s-1 3 L² mol-2 s-1 L mol-¹ S-1
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