Consider the reaction: 2 NO(g) + O2(g) NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] mol L-1 Initial [O2] mol L-1 Initial rate NO mol L-1s-1 Experiment 1 Experiment 2 Experiment 3 0.010 0.010 2.5 x 10-5 0.020 0.010 1.0 x 10-4 0.010 0.020 5.0 x 10-5 a. Determine the order of the reaction for each reactant. b. Write the rate equation for the reaction.

Consider the reaction: 2 NO(g) + O2(g) NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] mol L-1 Initial [O2] mol L-1 Initial rate NO mol L-1s-1 Experiment 1 Experiment 2 Experiment 3 0.010 0.010 2.5 x 10-5 0.020 0.010 1.0 x 10-4 0.010 0.020 5.0 x 10-5 a. Determine the order of the reaction for each reactant. b. Write the rate equation for the reaction.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...

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The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
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