Question

Nitrogen dioxide, a major air pollutant, can be produced by the combustion of nitrogen oxide as shown. 2NO O2 Right arrow. 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? Use Percent yield equals StartFraction actual yield over theoretical yield EndFraction times 100. 21. 7% 32. 6% 43. 5% 65. 2%.

Answer 1

Nitrogen dioxide is one of the primary components of air pollution. It is released by the combustion of nitrogen oxide.

How do you calculate the percentage yield of nitrogen oxide?

Given:

• Mass of nitrogen oxide consumed = 1500 kg
• Mass of nitrogen oxide produced = 1500 kg

The given chemical equation of nitrogen oxide is:

$\rm 2 NO + O_2 \rightarrow 2 NO_2$

Now, to calculate the percentage yield, the following conversion factor should be used:

$\rm 1500\; kg \;NO \times \dfrac{1000 \;g\; NO}{1\; kg \;NO}\times\dfrac {1 \;mol \;NO}{30\; g \;NO}\times\dfrac {2 \;mol \;NO_2}{2 \;mol \;NO}\times\dfrac {46 \;g \;NO_2}{1 \;mol \;NO_2}\times\dfrac {1 \;kg}{1000 \;g}$

Nitrogen dioxide = 2300 kg

The percentage yield will be:

$\rm Percentage Yield = \dfrac{Actual \; Yield}{Expected \;Yield}\times 100\\\\\\ \rm Percentage Yield = \dfrac{2500\;kg}{2300\;kg}\times 100$

Percentage yield = 65.2 %

Thus, the percentage yield of nitrogen dioxide is 65.2%.

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