Question

- 1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 11.7 M is : 2NH3(g) → N2(g) + 3H2(g) Suppose a vessel contains NH, at a concentration of 0.670 M. Calculate the concentration of NH, in the vessel 0.510 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x 6 ?

Answer 1

=> Solution . 2NH3(g) — Nalg) + 34449) ) Rate of disappearance of NH3 can be written as whert, Con Concentration of NHS dCA = K Ca 1 * Second-order kinetics is given Now, -da = kolt. 42 lat, t=0,G=640 - l Integraße t= t; G =CA Integraße I with proper fd Gw[Co-2] . kebet a 2 G . to = a la a to z kt] o iven a:- Rate constant, k = 11.7M!s time, t = OS10 sec. Juitial concentratim, Cso = 0.670 m. put all values in equation -

- ett bra om 19.22Sheos.se (5.967 t item) ant = 7.46 mi Therefore, CA = av 3 0.134 M thenes, com lenfraction of Nitts after 0.54 second is 0-13M 2-significant digits. 7.46
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