Question

5. Kcfor the following reaction is 0.212 at 100oC.N2O4(g)→2 NO2(g)A student running this reaction in the lab measures the concentrations as[N2O4] = 0.33 M and [NO2] = 0.66M. They conclude that the reaction must have reached equilibrium because there is a 2:1 ratio of products to reactants, just like in the balanced chemical equation. Decide if the student is right or wrong and explain your reasoning. If the student is right, prove they are right by verifying their conclusion. If the student is wrong, determine which direction the reaction will proceed to get to equilibrium.

Answer 1

Thanks

le given reaction is- N204 (8) ²2 N0g (8). ke at 10oc = 0.212. Nog] and [N₂o4] Expression of ke [No 2] 2 | the equilibrium [N, Oq ] concentration. At certain time, concentration of NO2 = 1 ntration of No2 = [no] = 0.66M) 0 0.04=[004] = 0.33m). " Reaction quotient (g) = [Nog] otient (a) = Where [Nog] and [ N204] are No2 and N204 respectively the at concentration of that time 16.66 so, 9= 0.4356 (0.337 0.33 - = 1.32 AS a ine o tk so the reaction is not reached at equilibrium. so, the student wan wrong As 8)K, so the reaction will shift toor toward left hand side ie rractant side to achive equilibrium.