121.0 g of NH3 is mixed with 207.1 g of O2 and allowed to react. The reaction is complete when the NH3 is consumed. 99.56 g of N2 is formed and 36.60 g O2 remain unreacted. What mass of H2O is produced? in grams
The balanced equation should be,
4 NH3 + 3 O2 -----------> 2
N2 + 6 H2O
First find out the limiting reactant,
moles of NH3 reacted = 121gm / 17.031 gm/mol = 7.1046
mol
moles of O2 reacted = (207.1-36.60)gm / 32 gm/mol =
5.3281 mol
Therefore O2 is the limiting reactant,
According to the reaction stoichiometry,
3 moles of O2 gives rise to 6 moles of
H2O
So, 5.3281 moles of O2 will give ? moles of
H2O
Cross multiply to get the answer,
(5.3281*6)/3 = 10.6562 mol of H2O are produced
Mass of H2O produced in grams = 10.6562mol *
18gm/mol = 191.8116 gms
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