Question

How many grams of potassium nitrate (KNO3) are required to produce 536 g of potassium nitrite (KNO2) according to the equation below?

2KNO3(s) ---> 2KNO2(s) + O2(g)

Answer 1

Answer on Question #50323, Chemistry, Other

Task:

How many grams of potassium nitrate (KNO₃) are required to produce 536 g of potassium nitrite (KNO₂) according to the equation below?

$$2 \mathrm{KNO_3}(s) \rightarrow 2 \mathrm{KNO_2}(s) + \mathrm{O_2}(g)$$

Answer:

$$\nu = \frac{m}{M}$$ $$M(\mathrm{KNO_2}) = 85\ \mathrm{g/mol}$$ $$M(\mathrm{KNO_3}) = 101\ \mathrm{g/mol}$$ $$\nu(\mathrm{KNO_2}) = \frac{536}{85} = 6.3\ \mathrm{mol}$$ $$\nu(\mathrm{KNO_2}) = \nu(\mathrm{KNO_3}) = 6.3\ \mathrm{mol}$$ $$m(\mathrm{KNO_3}) = \nu(\mathrm{KNO_3}) \cdot M(\mathrm{KNO_3})$$ $$m(\mathrm{KNO_3}) = 6.3 \cdot 101 = 637\ \mathrm{g}$$

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