0.89mol of NO is reacted with 0.5mol O2
NO + O2 2NO2
1. What are the coefficients that balance the reaction?
2. What is the limiting reactant?
3. What is the theoretical yield of NO2 (in grams)?
4. What is the actual yield if only 65% is produced?
2NO + O2 ----------------- 2NO2
For limiting reactant
2 mol of NO reacts with 1 mol of O2
0.89 mol reacts with (1*0.89)/2 mol of O2
= 0.445 mol
Total moles of O2 – reacted moles of O2=
remaining moles of O2
0.5mol – 0.445 mol = 0.055 mol remaining mol of O2
So, the limiting
reactant is NO
Theoretical yield of NO2
2NO = 2NO2
0.89 mol NO = 0.89mol NO2
Mass of NO2 = moles of NO2 * molecular
mass of NO2
= 0.89 * 46
= 40.94g NO2
ACTUAL YIELD OF NO2
Percent yield = (actual yield /theoretical yield)*100
65= (actual yield/40.94)*100
Actual yield = 26.611g
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