Salexirahusnagurul
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Consider the reaction for the production of NO2 from NO:
2 NO(g) + O2(g)¡2 NO2(g)
(a) If 84.8 L of O2(g) measured at 35 °C and 632 mm Hg, is allowed to react with 158.2 g of NO, find the limiting reagent.
(b) If 97.3 L of NO2 forms, measured at 35 °C and 632 mm Hg, what is the percent yield?

Draw a Lewis structure for each molecule and determine its molecular geometry. What kind of intermolecular forces are present in each substance?
(a) BCl3 (remember that B is a frequent exception t

Answer :

meerkat18
so now we use the number of moles of NO 5.27 moles. use again the PV=nRT R=62.36367(L mmHg K−1   mol−1) T=35C + 273 = 308K P=632 mm Hg V=97.3 L n=632*97.3/62.3636367*308=3.20145770868 Look at the mole ratio of NO to NO2 its 2:2 they share the same number of moles. Atomic weight of each element in NO2 N:14 O:16 Molar Mass:(16*2)+(14*1)=46 g Actual number of moles=3.20 Theortical number of moles=5.20 Percentage Yield=(Actual Yield/Theortical Yield)*100

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