A 10.0000 g block of aluminum is heated and placed in a stream of oxygen gas, resulting in the formation of aluminum oxide on the surface of the block.
The block is cooled and weighed and found to have a mass of 11.6471 g.
The block is then placed in a weak acid to remove the aluminum oxide layer from the block.
After a of the aluminum oxide is removed, the block is weighed and found to have a mass of 8.1471 g.
What is the empirical formula of aluminum oxide?
I know how to do the whole process for finding the empirical formula, but I am confused what is the mass of aluminum and what is the mass of oxygen that we start with?
I need to know this in order to multiply it by the molar mass.
I suggest you proof your post and correct the omission of word, or words, "After a ......of the aluminum...."
I don't understand what you mean?
I really need to know the values of aluminum and oxygen to solve the problem.
I guessed that Aluminum Oxide is 3.5 g and oxygen is 1.6471 g and Aluminum is 1. Something.
To determine the mass of aluminum and oxygen in the initial aluminum oxide compound, we can follow these steps:
1. Calculate the mass of aluminum in the block before any reaction occurs:
Mass of aluminum = Mass of block after reaction - Mass of aluminum oxide removed
Mass of aluminum = 11.6471 g - 8.1471 g = 3.5000 g
2. Since aluminum is a single element, its molar mass is equal to its atomic mass, which is 26.98 g/mol.
3. Now, to determine the mass of oxygen in the aluminum oxide compound, subtract the mass of aluminum from the mass of the block before any reaction:
Mass of oxygen = Mass of block before reaction - Mass of aluminum
Mass of oxygen = 10.0000 g - 3.5000 g = 6.5000 g
4. Oxygen is also a single element, and its atomic mass is 16.00 g/mol.
With this information, you can now calculate the moles of aluminum and oxygen, and subsequently determine the empirical formula of aluminum oxide.