If 16.00 g of O₂ reacts with 80.00 g NO, how many grams of NO₂ are produced? (enter only the value, round to whole number)

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

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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, the reaction is limited by the amount of available oxygen. 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.