the reaction for decomposition of dinitrogen monoxide gas to form oxygen radical
ID: 1005534 • Letter: T
Question
the reaction for decomposition of dinitrogen monoxide gas to form oxygen radicals is: N2o(g)->N2(g)+O(g). If thr rate constant k is 3.04x10^(-2) s^(-1) and the frequency factor, A is 8.00x10^(11) S^(-1), what is the activation energy for the first order reaction at 700C? (#6 I believe we us the formula 1/[At]=kt+1/[A0]) 2S203 solution in the first part of this experiment 3.What are the functons of solutions Kcr and s in this experiment? To maintain the ionic Srengtn of the 4. Wha soutions t is the purpose of using the CuS04 solution in this experiment? elp us identity the change in Raste 5. The following set of data was obtained by the method of initial rates for the reaction: 2 HgClz (aq) + Cz042. (aq) 2 Cll. (aq) + 2 COz (g) + Hg2Cl2 (s) What is the rate law for the reaction? Rate, M/se,0184-2 1.3 x 107 5.2 x 107 1.0 x 10-6 [HgCl2], M [C20421, M 22-4 0.10 0.10 0.20 0.10 0.20 0.20 6. The reaction for the decomposition of dinitrogen monoxide gas to form oxygen radicals is: N2O (g) N2(g) + 0 (g). If the rate constant, k, is 3.04 x 10-2 s1 and the frequency factor, A, is 8.00 x 1011 s-1, what is the activation energy for the first-order reaction at 700 oC? 7. Write an introduction of the experiment, your hypothesis for each of the parts of the experiment and a description of the procedure for each of the sections in the Procedure. Develop data tables for the information you need to collect in this 110 | P a geExplanation / Answer
6 .
K = Ae^-Ea/RT
K =3.04*10^-2 sec^-1
R = 8.314joule/mole-K
T = 700C = 700+273 = 973K
A = 8*10^11sce^-1
K = Ae^-Ea/RT
3.04*10^-2 = 8*10^11e^-Ea/8.314*973
3.8*10^-14 = e^-Ea/8089.52
log3.8*10^-14 = loge^-Ea/8089.52
-13.42 = -Ea/8089.52
Ea = 108561.35 joules = 108.56135kj >>>> answer
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