Jump to. 10/16/2017 11:55 PM 12.2/10010/16/2017 12:58 PM Print·Calculator Period

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Jump to. 10/16/2017 11:55 PM 12.2/10010/16/2017 12:58 PM Print·Calculator Periodic Table Gradebook Question 9 of 23 General Chemistry 4th Edition University Science Books presented by Sapling Learming Map t At a certain temperature, the equilibrium constant for the following chemical equation is 3.20, De Po At this temperature, calculate the number of moles of NO-g) that must be added to 2.42 mol af SOx(o) in order to form 1.10 mol of SO3(g) at equilibrium. You You give You c until y You lo Number mol of No,l) O eTexth 0 O Help w 0 O Web Help O Technical S 0 Previous Give Up & iew Sousion Check Answer NextExt

Explanation / Answer

FROM equation ,

   SO2(g) + NO2(g) <---> SO3(g) + NO(g)

initial 2.42 mol    x Mol          0 Mol   0 Mol

change   -1.1       -1.1          +1.1       +1.1

equili   1.32 mol   x-1.1 mol      1.1 mol   1.1 mol

Kc = [SO3][NO]/[SO2][NO2]

3.2 = (1.1*1.1)/(1.32*(x-1.1))

x = 1.39

no of mol of NO2 must be added = 1.39 mol

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