How would you solve this one?

Question

Consider the following equation

4Al(s)+3O2(g)>2Al2O3(s)

How many moles of Al2O3 can be produced from the reaction of 10.0g of Al and 19.0 g of O2?

Answer 1

You need the molar mass of each of the compoenents

Al = 26.98 g/mol so you have 10/26.98 moles of Al = 0.37 mols

O2 = 2*(16) g/mol so you have 19/(2*16) moles of O2= 0.59 mols

The ratio of use of Al to O2 is 4/3 so you will have an excess of O2 in this equation and Al is the limiting factor

For every 4 mols of Al you get 2 moles of Al2O3, so it is a 2/1 relationship

Since you have a 0.37 moles of Al you get 0.37/2 moles of product = 0.185 or so