Question 2 Calculate The Rate Law Constant K Based On The Reactant Orders And Experimental Data Below Do Not Include 1 (94.2 KiB) Viewed 29 times
Question 2 Calculate the rate law constant, k, based on the reactant orders and experimental data below. Do not include units in your answer. Question 3 Experiment 1 2 A + B + C + D + E Reactant Order [A]。 (M) 0.35 。 (M) 0.29 A B C 2 1 2 [C]。 (M) 0.36 A + 3 B 2 C Initial Rate 10 pts 0.0154 M/min 10 pts Two gases, A and B, are placed in an empty, 3.98-liter container at 500 °C. When equilibrium is established, 3.44 mol A, 2.62 mol B, and 0.94 mol C are present. Evaluate Kc for the following reaction at 500 °C. Question 1 Given the following data, determine the rate-law expression and the value of the rate constant for the reaction (k), and the units of k. Experiment 1 2 32 4 [A]。 (M) 0.20 M 0.40 M 0.20 M 0.20 M Rate Constant: 2 A + B + C →D + E Units: 。 (M) 0.20 M 0.30 M 0.30 M Rate Law Expression: 0.40 M [C]。 (M) 0.20 M 0.20 M 0.20 M 0.60 M Initial Rate 10 pts M-min 2.4 x 10-6 9.6 x 10-6 M min-1 -6 2.4 x 10 M.min -1 -1 7.2 x 10-6 M min-¹
D Question 7 10 pts How much NH4Cl (in grams) must be added to 2.00 liters of 0.21 M aqueous ammonia to give a solution with pH = 8.55? Do not include units in the answer blank. Assume no volume change due to the addition of NH4Cl. The K of ammonia is 1.8 x 10-5, and the molar mass of ammonium chloride is 53.491 g/mol
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