Answer:
94.16g of N2O
50.88g of O2
Explanation:
O2 reacts with N2 as follows:
2N2 + O2 → 2N2O
To find moles of N2O produced we need to convert the mass of each gas to moles to find limiting reactant and the moles of N2O that could be produced:
Moles N2 (Molar mass: 28g/mol):
60g N2 * (1mol / 28g) = 2.14 moles N2
Moles O2 (Molar mass: 32g/mol):
85g O2 * (1mol / 32g) = 2.66 moles O2
For a complete reaction of 2.14 moles of N2 are needed:
2.14 mol N2 * (1mol O2 / 2 mol N2) = 1.07 moles of O2.
As there are 2.66 moles of O2, reactant in excess is O2 and will remain:
2.66 moles - 1.07 moles =
1.59 moles O2. The mass is:
1.59 moles O2 * (32g / mol) =
And there are produced:
2.14 mol N2 * (2 moles N2O / 2 moles N2) = 2.14 moles N2O.
The mass is (44g/mol for N2O):
2.14 moles N2O * (44g/mol) =
