Question

assume that coal can be represented by the chemical formula c135h96o9ns . if 2.00 tons of coal is burned, what mass of nitrogen in the form of nox gases, is produced by this combustion?

Answer 1

If 2.00 tons of coal is burned, then the mass of nitrogen in the form of nox gases, is produced by this combustion is 400134 g of nitrogen.

The chemical reaction equation can be written as

C135H96O9NS + 156O2 ------- 135CO2 + 48H2O + NO + SO2

Mass of 2.0 tons of coal in gram = 1.814 × 10^(6) g

Molar mass of C135H96O9NS can be calculated as = 135(12) + 96(1) + 14 + 32 = 1904 moles of coal

Now, number of moles of coal burned = 1.814 × 10^(6) g / (1906 g/mol) = 952.7 moles of coal

If 1 mole of coal produced 1 mole of NO

Total 952.7 moles of coal produced 952.7 moles of NO

Mass of NO can be calculated as

Mass of NO produced = 952.7 × 30 = 28581 g

1 mole of NO = 30 g of NO

Thus, 14 g of nitrogen is contained in 30 g of NO

Let xg of nitrogen is contained in 28581 g of NO

Then,

x = 14 × 28581 = 400134 g of nitrogen.

If 2.00 tons of coal is burned, then the mass of nitrogen in the form of nox gases, is produced by this combustion is 400134 g of nitrogen.

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