Question

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

Answer 1

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Answer 2

Answer:0.28975 moles of nitrogen are formed .

Explanation:

$4KNO_3(s)\rightarrow 2K_2O(s)+2N_2(g)+5O_2(g)$

Number of moles of $KNO_3=\frac{\text{Mass of the}KNO_3}{\text{Molar mass of the}KNO_3}=\frac{58.6 g}{101.11 g/mol}=0.5795 moles$

According to reaction , 4 mol of $KNO_3$ produces 2 moles of $N_2$ gas.

Then,0.5795 moles of $KNO_3$ will produce=$\frac{2}{4}\times 0.5795$ moles of $N_2$ gas:

$\frac{2}{4}\times 0.5795=0.28975 moles$

0.28975 moles of nitrogen are formed.