Nitrogen dioxide, a major air pollutant, can be produced by the combustion of nitrogen oxide as shown.
2no + o2 > 2no2
in a plant, 1,500 kg of nitrogen oxide is consumed per day to produce 1,500 kg of nitrogen dioxide per day. what is the percent yield?
21.7%
32.6%
43.5%
65.2%

Answer is: the percent yield is 65.2%.

Balanced chemical reaction: 2NO + O₂ → 2NO₂.

m(NO) = 1500 kg; mass of nitrog oxide.

From balanced chemical reaction: n(NO) : n(NO₂) = 2 : 2 (1 : 1).

m(NO) : M(NO) = m(NO₂) : M(NO₂).

1500 kg : 30 g/mol = m(NO₂) : 46 g/mol.

m(NO₂) = 1500 kg · 46 g/mol ÷ 30 g/mol.

m(NO₂) = 2300 kg.

the percent yield = 1500 kg ÷ 2300 kg · 100%.

the percent yield = 65.21%.

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