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________ Finding the remaining parts. Mass of oxygen in oxide product ________________ Moles of magnesium. (show calculation) ________________ Moles of oxygen. (show calculation) ________________
Given the following data, answer the remaining questions.
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______18.500_____ |
|
________18.702________ |
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Mass of Mg |
________0.202________ |
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Mass of crucible +cover+ oxide product |
________18.842____ |
|
Mass of oxide product |
________0.342________ |
Finding the remaining parts.
|
Mass of oxygen in oxide product |
________________ |
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Moles of magnesium. (show calculation)
|
________________
|
|
Moles of oxygen. (show calculation)
|
________________
|
|
Empirical formula of oxide product. (Show calculations) |
________________ |
Then answer these questions, please show work.
- How many grams of nitrogen are in 1.50g of Mg3N2?
- What is the empirical formula of a compound that is made up of 81.68% carbon and 18.32% hydrogen?
- Upon combustion, a 0.8009 g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6004g CO2 and 0.6551g H2O. Find the empirical formula of the compound.
Here is some information to help.
In this experiment, magnesium metal is heated until it reacts with oxygen in the air according to the following balanced equation:
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2Mg(s)+ O2(g) → 2MgO(s) |
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(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.
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3Mg(s)+ N2(g) → Mg3N2(s) |
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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.
Since you have posted a question with multiple sub-parts, we will solve the first three subparts for you. To get the remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.
Given data:
|
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_______ |
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