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3 years ago

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)

Chemistry

1 answer:

Norma-Jean [14]3 years ago

6 0

Answer:

46 g

Explanation:

The balanced equation of the reaction between O and NO is

2 NO + O₂ ⇔ 2 NO₂

Now, you need to find the limiting reagent. Find the moles of each reactant and divide the moles by the coefficient in the equation.

NO: (80 g)/(30.006 g/mol) = 2.666 mol

(2.666 mol)/2 = 1.333

O₂: (16 g)/(31.998 g/mol) = 0.500 mol

(0.500 mol)/1 = 0.500 mol

Since O₂ is smaller, this is the limiting reagent.

The amount of NO₂ produced will depend on the limiting reagent. You need to look at the equation to determine the ratio. For every mole of O₂ reacted, 2 moles of NO₂ are produced.

To find grams of NO₂ produced, multiply moles of O₂ by the ratio of NO₂ to O₂. Then, convert moles of NO₂ to find grams.

0.500 mol O₂ × (2 mol NO₂/1 mol O₂) = 1.000 mol NO₂

1.000 mol × 46.005 g/mol = 46.005 g

You will produce 46 g of NO₂.

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