What Mass Of Copper(i)oxide Is Formed By Burning 10.5g Of Copper(i)sulfide
To determine the mass of copper(I) oxide formed by burning 10.5g of copper(I) sulfide, you need to first calculate the balanced chemical equation for the reaction between copper(I) sulfide (Cu2S) and oxygen (O2).
The balanced chemical equation for this reaction is as follows:
2Cu2S + 3O2 -> 2Cu2O + 2SO2
From the balanced equation, you can see that 2 moles of Cu2S react with 3 moles of O2 to produce 2 moles of Cu2O.
Now, let's calculate the molar mass of Cu2S and Cu2O:
Molar mass of Cu2S:
1 Copper atom = 63.55 g/mol
2 Sulfur atoms = 32.07 g/mol x 2 = 64.14 g/mol
Total molar mass of Cu2S = 63.55 g/mol + 64.14 g/mol = 127.69 g/mol
Molar mass of Cu2O:
2 Copper atoms = 63.55 g/mol x 2 = 127.1 g/mol
1 Oxygen atom = 16.00 g/mol
Total molar mass of Cu2O = 127.1 g/mol + 16.00 g/mol = 143.1 g/mol
Now, let's calculate the amount of Cu2O formed:
10.5 g of Cu2S / (127.69 g/mol) x (2 mol Cu2O / 2 mol Cu2S) x (143.1 g/mol) = 11.8 g of Cu2O
Therefore, approximately 11.8 grams of copper(I) oxide (Cu2O) is formed by burning 10.5 grams of copper(I) sulfide (Cu2S).