The gas-phase conversion of nitric oxide and hydrogen to nitrogen and water follows the reaction Select one: v=k(PNO)² k NO(g) + H₂(g) → ½ N₂(g) + H₂O(g) Po H₂ (kPa) 53.3 53.3 38.5 19.6 The rate of production of nitrogen as a function of initial reactant pressures is shown in the table at right. What is the rate law for this reaction? Can't tell from the information given v = k(PNO) (PH2) v=k(PNO) ² (PH2) v = k(PNO) (PH2)² Run 1 2 3 4 Po NO (kPa) 40.0 20.3 53.3 53.3 Rate (kPa/s) 0.137 0.033 0.213 0.105

The gas-phase conversion of nitric oxide and hydrogen to nitrogen and water follows the reaction Select one: v=k(PNO)² k NO(g) + H₂(g) → ½ N₂(g) + H₂O(g) Po H₂ (kPa) 53.3 53.3 38.5 19.6 The rate of production of nitrogen as a function of initial reactant pressures is shown in the table at right. What is the rate law for this reaction? Can't tell from the information given v = k(PNO) (PH2) v=k(PNO) ² (PH2) v = k(PNO) (PH2)² Run 1 2 3 4 Po NO (kPa) 40.0 20.3 53.3 53.3 Rate (kPa/s) 0.137 0.033 0.213 0.105

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

Section11.1: Reaction Rate

Problem 11.3CE

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