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.

hurricanes form when warm, moist air from the ocean surface quickly rises into the atmosphere and forms storm clouds and rain. when the clouds are formed, heat is released which warms the cool air in the upper regions of the atmosphere so that the cycle can continue. which two phases of the water cycle are repeated in this process?