Question

Assume that coal can be represented by the chemical formula C135H96O9NS. If 4.0 tons of coal is burned, what mass of nitrogen is found in the NO produced by this process?

Answer 1

Answer:

0.02 tons of NO produced when 4 tons of coal is burned

Explanation:

From the given,

Chemical formula of coal =  $C_{134}H_{96}O_{9}NS$

Molecular mass of coal = $(134\times12)+(9\times1)+(9\times16)+14+32\,=1906.1gm$

Let’s calculate the mass of nitrogen in coal

$Percentage\,weight\,of\,nitrogen=\frac{Mass\,of\,nitrogen}{Molecular\,mass\,of coal}$

$Percentage\,weight/,of/,nitrogen=\frac{14}{1906.1}=0.73%$

Amount of coal burnt = 4tons

Amount of NO produced by burning 4tons = $4\,tons\,of\,coal\times \frac{0.73tons}{100\,tons\,of\,coal}=0.0292\,tons$

This nitrogen is converted into NO by reacting with atmospheric oxygen.

Answer 2

Answer:

26653.9 grams of nitrogen is found in the nitrogen dioxide produced by this process.

Explanation:

$C_{135}H_{96}O_9NS + \frac{313}{2}O_2\rightarrow 135CO_2 + 48H_2O+ NO_2 + SO_2$

Mass of the coal = 4.0 tons  

1 ton = 907185 g

$4.0 tons = 4\times 907185g=3,628,740 g$

Molar mass of coal = 1,906 g/mol

Moles of coals = $\frac{3,628,740 g}{1,906 g/mol}=1,903.85 mol$

According to reaction,  1 mole of coal gives 1 mole of nitrogen dioxide gas.

Then, 1,903.85 mole of coal on combustion will give:

$\frac{1}{1}\times 1,903.85 mol=1,903.85 mol$ of nitrogen dioxide gas

1 mole of nitrogen dioxide gas has 1 mole of nitrogen atom.Then 1,903.85 moles of nitrogen dioxide will have ;

$1\times 1,903.85 mol=1,903.85 mol$ of nitrogen

Mass of 1,903.85 moles of nitrogen dioxide gas :

1,903.85 mol × 14 g/mol = 26653.9 g

26653.9 grams of nitrogen is found in the nitrogen dioxide produced by this process.