Question

Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) → N2 (g) + H20 (1) AWNA Experiment (NH4+1: [NO2). Initial rate (M/s) 0.24 0.10 17.2 x 10-4 0.12 0.10 13.6 x 10-4 0.15 15.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH4+] at 103 seconds after the start of the reaction. In this experiment, both reactants are present at the same initial concentration. The units should be M, and should be calculated to three significant figures. .119 M This reaction is first order in both reactants. In Experiment4, the initial concentration are the same for both reactants. Since they react in a one-to-one ratio, this can be represented as a second order reaction of the type rate = k[A]2 The integrated rate law is: 1/[A]= kt + 1/[A]. Submit Answer Incompatible units. No conversion found between "m" and the required units. Tries 12/45 Previous Tries

Answer 1

Ret Rate All K (0.24 0.lo) - © Let Rate = K[NHU][NO] from exp-1) 7.2x104 = K (0.24)*(0.10% 0 from exp-(2) 3.68104 = K (0.12) & (0.104 - from eaf-3) 504x104-K (0.12)?(0.1517 © on dividing 04 ©, 7.2 - 10.2412 » 2-(2) QC=D on dividing di 3Con este C:): Jy s kamen - (0.66)' o 9 0.66

from 0 & Rate = k [NHut] '[NO] = 3x10²=0.03 M's & Here reaction is of first order with respect to both the reactants K= 0.24) (0-10)