Question

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 1

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%.

Answer 2

Percent yield is calculated by obtaining the ratio of the actual yield and the theoretical yield times 100.

Actual yield = 1500 kg

Theoretical yield = 1500 ( 1 / 30.00 ) ( 2 / 2 ) ( 46.006 / 1 ) = 2300.3 kg

Percent yield = 1500 / 2300.3 x 100 = 65.21 %

Therefore, the correct answer is the last option. Hope this answers the question.