1.Solid iron (III) oxide can be formed by heating solid magnesium oxide in the p

Question

1.Solid iron (III) oxide can be formed by heating solid magnesium oxide in the presence of solid metallic iron. The byproduct of the reaction is solid metallic magnesium. Balance the reaction described. Use appropriate chemical formulas. Include states of matter.

2.Determine the number of grams of magnesium oxide needed to produce 30.0 g of iron (III) oxide.

3.Automotive air bags inflate when sodium azide (NaN3) decomposes explosively to its constituent elements. How many grams of sodium azide are required to produce 33.7 g of nitrogen?

Explanation / Answer

1) 3MgO (s) + 2Fe (s) -------> Fe2O3 (s) + 3Mg (s)

2) Mass of iron (III) oxide = 30 g

Molar mass of iron (III) oxide = 159.7 g / mol

=> Moles of iron (III) oxide = 30 / 159.7 = 0.188 moles

According to the stoichiometry of the reaction 3 moles of MgO produces 1 mole of iron (III) oxide

=> Moles of MgO required = 0.188 x 3 = 0.564 moles

Molar mass of MgO = 40.3044

=> Mass of MgO = 0.564 x 40.3044 = 22.72 g

3) 2 NaN3 (s) -----> 2Na (s) + 3 N2 (g)

Mass of N2 required = 33.7 g

molar mass of N2 = 28

=> Moles of N2 = 33.7 / 28 = 1.204 moles

According to the stoichiometry of the reaction 2 moles of NaN3 produces 3 moles of N2

=> Moles of NaN3 required = 1.204 x 2 / 3 = 0.803 moles

Molar mass of NaN3 = 65 g / mol

=> Mass of NaN3 = 0.803 x 65 = 52.195 g

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