72KINE 505: Studying the Rate of Reaction of Potassium Permanganate and Oxalic Acid4. Consider the reaction of ammonium ions (NH+) and nitrite ions (NO,), shown in Equation 19.NH,(aq) + NO, (aq) → N2(g) + 2 H20(1)(Eq. 19)Solutions containing NH and NO, were mixed in various quantities and the following rate data at a constanttemperature were obtained:initial NHconcentration,initial NO2initial rate fordeterminationconcentration,formation of N2bnumbermol/Lmol/Lmol/L's7.50 x 10-31.50 x 10-21.50 x 10-23.04 x 10-76.08 x 10-71.22 x 10-610.1500.150ap30.300(a) Use the method of initial rates to find the or-der of the reaction with respect to NH*.(c) Calculate the rate constant, k, for the reactionof NH,* and NO2.shi(d) Write the rate equation for the reaction ofNH,* and NO,.Use the method of initial rates to find the order(b)of the reaction with respect to NO2.

Answer: Order of reaction with respect to each reactant is actually its molecularity in the rate…

4. Consider the reaction of ammonium ions (NH*) and nitrite ions (NO,"), shown in Equation 19. NH,*(aq) + NO," (aq) → N2(g) + 2 H20(!) (Eq. 19) Solutions containing NH,* and NO, were mixed in various quantities and the following rate data at a constant temperature were obtained: initial NO2 initial rate for initial NH concentration, determination concentration, formation of N2 number moVL mo/L mol/L's 7.50 × 10-3 1.50 x 10-2 1.50 x 10-2 3.04 x 10-7 6.08 x 10-7 1.22 x 10-6 0.150 0.150 0.300 (c) Calculate the rate constant, k, for the reaction of NH,* and NO,. (a) Use the method of initial rates to find the or- der of the reaction with respect to NH. (b) Use the method of initial rates to find the order of the reaction with respect to NO2. (d) Write the rate equation for the reaction of NH, and NO,.

4. Consider the reaction of ammonium ions (NH) and nitrite ions (NO,"), shown in Equation 19. NH,(aq) + NO," (aq) → N2(g) + 2 H20(!) (Eq. 19) Solutions containing NH,* and NO, were mixed in various quantities and the following rate data at a constant temperature were obtained: initial NO2 initial rate for initial NH concentration, determination concentration, formation of N2 number moVL mo/L mol/L's 7.50 × 10-3 1.50 x 10-2 1.50 x 10-2 3.04 x 10-7 6.08 x 10-7 1.22 x 10-6 0.150 0.150 0.300 (c) Calculate the rate constant, k, for the reaction of NH,* and NO,. (a) Use the method of initial rates to find the or- der of the reaction with respect to NH. (b) Use the method of initial rates to find the order of the reaction with respect to NO2. (d) Write the rate equation for the reaction of NH, and NO,.

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

Section11.7: Reaction Mechanisms

Problem 11.12E

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