Question

Please answer the following question

72 KINE 505: Studying the Rate of Reaction of Potassium Permanganate and Oxalic Acid 4. Consider the reaction of ammonium ions (NH4') and nitrite ions (NO2),shown in Equation 19. NH4 (aq)+NO2 (aq) N2(9)+2 H2OU) Eq. 19) Solutions containing NH4 and NO2 were mixed in various quantities and the following rate data at a constant temperature were obtained: determination number initial NH4 concentration, mol/L initial NO2 concentration mol/L initial rate for formation of N2 molL.s 0.150 0.150 0.300 7.50 x 10-3 1.50 x 10-2 3.04 x 107 6.08 x 10-7 1.22 x 10-6 Calculate the rate constant, k, for the reaction 1.50 x 10-2 (a) Use the method of initial rates to find the or- der of the reaction with respect to NH4 (c) of NH4 and NO2

Answer 1

Let the rate law of the equation be rate, r = K[NH^+_4]^x [NO^-_2]^y To find x and y and x + y. It is asked to give the value of x. based on the given date write the rate laws for three tricks rightarrow (1) 3.04 times 10^-7 m/s = K(0.150 m)^x(7.5 times 10^-3m)^y (2) 6.06 times 10^-7 m/s = k (0.150m)^x (1.5 times 10^-2 m)^x (3) 1.22 times 10^-6 m/s = k (0.300 m)^x (1.5 times 10^-2 m)^y now (2)/(1) 6.06 times 10^-7 m/s/3.04 times 10^-7 m/s = 2 = 2 y = 1 (3)/(2) 1.22 times 10^-6 m/s 6.07 times 10^-7 m/s x = 1 \r\n so order of the reaction w.r.tntt is 1 To determine k consider any one of the 3 equations. 3.04 times 10^-7 m/s = k (0.150)^1(7.5 times 10^-3m)^1 k = 3.04 times 10^-7 m/s/(0.150m)(7.5 times 10^-3m) k = 2.702 times 10^-4 m^-1 s^-1