how many grams of H2O are produced from the complete reaction of 68.12 g of NH3 ?

Question

NH3 + O2 → NO + H2O

If the percent yield of the above reaction is found to be 94.20 %

Answer 1

First, balence the reaction equation:
4NH3 + 5O2 → 4NO + 6H2O
So 4 moles NH3 reacts to produce (theoretically) 6 moles of H2O.
The molar mass of NH3: 17.03 g/mol
The molar mass of H2O: 18.02 g/mol
68.12g NH3 <==> 4.000 mol NH3 ==> 6.000 mol H2O <==> 108.1g H2O
108.1g * 94.20 % = 101.8g.

Answer 2

First you may stability the reaction equation NH3 + 5/4 O2 -> NO + 3/2 H2O ok so the multipliers at the instant are not integers. in simple terms multiply all numbers by ability of four. in spite of the shown fact that this type is greater usefull to your difficulty. Then the atomic weight of NH3 is 17. So there are 17 grams in keeping with mole. So now all of us understand there are sixty 8.12/17 = 4 Moles of NH3 , consequently there are 6 Moles of H2O produced. by way of fact the atomic weight of H2O is eighteen, there are 6 * 18 = 108 grams of H2O produced.