Salexirahusnagurul
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Consider the reaction for the production of NO2 from NO:

2 NO(g) + O2(g)¡2 NO2(g)

AIf 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.
BIf 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?

ABCl3 (remember that B is a frequent exception t

Verified 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=63297.3/62.3636367308=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:(162)+(141)=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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