Answer:
84 g
Explanation:
The molecular weight of nitrogen is 14.01 g/mol. That of oxygen is 16.00 g/mol, so the weights of the various elements available are ...
From NO
N: (14.01/(14.01+16.00))·(80 g) = 37.35 g
O: 80 g -37.35 g = 42.65 g
From O₂
O: 16 g
__
In each mole of NO₂, the weight of the oxygen is 2(16.00) = 32 g. The weight of the nitrogen is 1(14.01) = 14.01 g.
From the available oxygen, we can produce ...
(42.65 g +16 g)/(32.00 g/mol) = 1.83 mol of NO₂
From the available nitrogen, we can produce ...
(37.35 g)/(14.01 g/mol) = 2.67 mol of NO₂
Clearly, <em>the reaction is limited by the amount of available oxygen</em>. Then the mass of the NO₂ that can be produced is ...
(1.83 mol)(32.00 +14.010 g/mol = 84.3 g ≈ 84 g.
84 grams of NO₂ are produced.
