Angel Iwu_Det. rate laws & orders.worksheet

Activities and Explorations: 10 points, Due Sunday April 2, 11:59 PM Determine Rate Laws and Orders Instructions: Upload your work on this page to Brightspace by typing or writing your responses and saving the file and uploading that file as a pdf (not HEIC or pages). You can also take pictures of your written work and paste them in! Learning Objectives 13.2 The Rate Law • Find the rate law of a reaction given experimental data. 1. Consider the reaction 2 NO (g) + 2 H 2 (g) ® N 2 (g) + 2 H 2 O (g). From the data in the table below determine the following: Experiment Rate, (M/s) [NO], (M) [H 2 ], (M) 1 1.25 ´ 10 − 5 5.00 ´ 10 − 3 2.00 ´ 10 − 5 2 5.00 ´ 10 − 5 10.00 ´ 10 − 3 2.00 ´ 10 − 5 3 10.00 ´ 10 − 5 10.00 ´ 10 − 3 4.00 ´ 10 − 5 A. The rate law (meaning find Rate = k[NO] x [H 2 ] y , and determine x and y.) r = k [H 2 ] 1   [NO] 2 B. The rate constant (once you have the rate law, determine what k is). K= 2.5 x 10 ^4 M ^-2 s^-1 C. Is the order of NO and the order of H 2 related to the stoichiometric coefficients in the balanced chemical equation? Explain why or why not. The order of reaction is the sum of the powers raised by the reactant quantity in the rate laws equation. It is defined as the degree to which the overall rate is impacted by a change in the quantity of substance. They are not related to the stoichiometric coefficients because as stated in lecture if they relate there may be a fluke. 2. Consider the reaction 2 NO 2 (g) + F 2 (g) ® 2 NO 2 F (g). From the data in the table below determine the following: Experiment Rate, (M/s) [NO 2 ], (M) [F 2 ], (M) 1 0.026 0.100 0.100 2 0.051 0.200 0.100 3 0.103 0.200 0.200 4 0.411 0.400 0.400 A. The rate law (meaning find Rate = k[NO 2 ] x [F 2 ] y , and determine x and y.) k[NO 2 ] 1 [F 2 ] 1