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20.Use the following data to determine the reaction rate law for the system. Be sure to solve for the rate law constant as well including its units for full marks NO(g) + H2(g) →→→→→→HNO2(g) Experiment 1 2 3 4 5 6 NO (mol/L) 0.001 0.002 0.003 0.004 0.004 0.004 H2 (mol/L) 0.004 0.004 0.004 0.001 0.002 0.003 Initial Rate of Reaction (mol/(L.s)) 0.004 0.0016 0.036 0.016 0.032 0.048

20.Use the following data to determine the reaction rate law for the system. Be sure to solve for the rate law constant as well including its units for full marks NO(g) + H2(g) →→→→→→HNO2(g) Experiment 1 2 3 4 5 6 NO (mol/L) 0.001 0.002 0.003 0.004 0.004 0.004 H2 (mol/L) 0.004 0.004 0.004 0.001 0.002 0.003 Initial Rate of Reaction (mol/(L.s)) 0.004 0.0016 0.036 0.016 0.032 0.048

Chemistry
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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20. Use the following data to determine the reaction rate law for the system. Be sure to solve for the rate law constant as well including its units for full marks NO + H2(g) →HNO, Experiment 1 2 3 4 5 6 (2(g) NO (mol/L) 0.001 0.002 0.003 0.004 0.004 0.004 H2 (mol/L) 0.004 0.004 0.004 0.001 0.002 0.003 Initial Rate of Reaction (mol/(L.s)) 0.004 0.0016 0.036 0.016 0.032 0.048
Transcribed Image Text:20. Use the following data to determine the reaction rate law for the system. Be sure to solve for the rate law constant as well including its units for full marks NO + H2(g) →HNO, Experiment 1 2 3 4 5 6 (2(g) NO (mol/L) 0.001 0.002 0.003 0.004 0.004 0.004 H2 (mol/L) 0.004 0.004 0.004 0.001 0.002 0.003 Initial Rate of Reaction (mol/(L.s)) 0.004 0.0016 0.036 0.016 0.032 0.048
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