here is some information to help in this experiment magnesium metal is heated until it reacts wi

First, we need to find the mass of oxygen in the oxide product. We can do this by subtracting th

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In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation: 2Mg(s) + O2(g) → 2MgO(s) (silver metal) (white-gray ash) As the magnesium burns in air, it may also combine with nitrogen in the air. To remove any nitride product, water is added, and the product is reheated. Any nitride product is converted to magnesium oxide and ammonia. 3Mg(s) + N2(g) → Mg3N2(s) Mg3N2(s) + 3H2O(l) → 3MgO(s) + 2NH3(aq) A weighed amount of the magnesium metal is used, and the mass of the oxide product formed is determined at the end of the experiment. The mass of oxygen that combines with the magnesium is obtained from the difference between the mass of the oxide product and the original mass of magnesium. mass of oxide product - mass of magnesium = mass of oxygen in oxide product The empirical formula of the oxide product is determined by calculating the moles of magnesium and the moles of oxygen using their respective molar masses. Dividing the moles of the elements by the smaller number of moles gives the empirical formula. Given the following data, answer the remaining questions. Mass of crucible + cover: 18.500 Mass of crucible + cover + Mg: 18.702 Mass of Mg: 0.202 Mass of crucible + cover + oxide product: 18.842 Mass of oxide product: 0.342 Find the remaining parts. Mass of oxygen in oxide product: Moles of magnesium (show calculation): Moles of oxygen (show calculation): Empirical formula of oxide product (show calculations):

          In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation:
2Mg(s) + O2(g) → 2MgO(s)
(silver metal) (white-gray ash)

As the magnesium burns in air, it may also combine with nitrogen in the air. To remove any nitride product, water is added, and the product is reheated. Any nitride product is converted to magnesium oxide and ammonia.
3Mg(s) + N2(g) → Mg3N2(s)
Mg3N2(s) + 3H2O(l) → 3MgO(s) + 2NH3(aq)

A weighed amount of the magnesium metal is used, and the mass of the oxide product formed is determined at the end of the experiment. The mass of oxygen that combines with the magnesium is obtained from the difference between the mass of the oxide product and the original mass of magnesium.
mass of oxide product - mass of magnesium = mass of oxygen in oxide product

The empirical formula of the oxide product is determined by calculating the moles of magnesium and the moles of oxygen using their respective molar masses. Dividing the moles of the elements by the smaller number of moles gives the empirical formula.

Given the following data, answer the remaining questions.

Mass of crucible + cover: 18.500
Mass of crucible + cover + Mg: 18.702
Mass of Mg: 0.202
Mass of crucible + cover + oxide product: 18.842
Mass of oxide product: 0.342

Find the remaining parts.

Mass of oxygen in oxide product: ________________
Moles of magnesium (show calculation): ________________
Moles of oxygen (show calculation): ________________
Empirical formula of oxide product (show calculations): ________________

Added by William S.

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