The rate law for the reaction 2NO(g) + 2H₂(g)N₂(g) + 2H₂O(g) israte = K[NO]²[H₂]-1If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ whenthe concentrations of NO and H₂ are both 6.9 x 10-6mol L-¹, what is the value of the rate constant andwhat are the units for the rate constant?k=ix 1013X9.565-1mol L-¹5-1L³ mol-³ s-13L² mol-2 s-1L mol-¹ S-1

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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

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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