What mass of nitrogen is formed by burning 11.2 liters of ammonia?

To solve it, you need to compose the reaction equation:
4NH3 + 2O2 = 2N2 + 6H2O – ammonia combustion reaction, nitrogen and water were obtained;
Let’s calculate the molar masses of substances:
M (NH3) = 14 + 1 * 3 = 17 g / mol;
M (N2) = 14 * 2 = 28 g / mol;
Let’s determine the amount of moles of ammonia, if its volume is known:
1 mol of gas at n. y occupies a volume of 22.4 liters;
X mol (NH3) -11.2 l. hence, X mol (NH3) = 1 * 11.2 / 22.4 = 0.5 mol;
Let’s make a proportion according to the equation:
0.5 mol (NH3) – X mol (N2);
-4 mol -2 mol hence, X mol (N2) = 0.5 * 2/4 = 0.25 mol;
We find the mass of nitrogen by the formula:
m (N2) = Y * M = 0.25 * 28 = 7 g.
Answer: in the process of the ammonia combustion reaction, nitrogen with a mass of 7 g was released.