NH3 + O2 → NO + H2O how many grams of NO are produced from the complete reaction of 64.00 g o2

Answer 1

Balance the Equation
4NH3 + 5O2 --> 4NO + 6H2O

Convert from g O2 to moles O2

(64.00 g O2) * (1 mol O2)/(32.00 g) = 2 mol O2

Convert from moles O2 to moles NO

(2 mol O2) * (4 mol NO)/(5 mol O2) = 1.6 mol NO

Convert from moles NO to grams NO

but first we need to figure out NO's molecular weight

1 mol N * 14.01g/mol = 14.01g
1 mol O * 16.00g/mol = 16.00g
30.01g/mol NO

Now we can continue

1.6 mol NO * 30.01g/mol = 48.02 g NO produced

Hope this helps!

Answer 2

Balance the equation
4NH3 + 5O2 ==> 4NO + 6H2O
so 64 g of O2 are produced and the ratio is 5 mols of O2 react to make 4 moles of NO
64g/32 is 2 moles of O2 and so using a 5:4 mol ratio you can find the number of moles of NO then the grams
so 1.6 moles of NO are produced which is the molar mass of NO (14.01+16) = 30.01g times 1.6 moles = 48.016g of NO are produced