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 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 Empirical formula of oxide product.
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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 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.
|
______18.500_____ |
|
________18.702________ |
|
Mass of Mg |
________0.202________ |
|
Mass of crucible +cover+ oxide product |
________18.842____ |
|
Mass of oxide product |
________0.342________ |
Find the Empirical formula of oxide product.
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