Consider the chemical equation.
4NH3+5O2⟶4NO+6H2O4NH3+5O2⟶4NO+6H2O
When 26 g of ammonia burn in 26 g of oxygen, what is the limiting reagent?
NH3NH3 and O2O2
NONO
O2O2
H2OH2O
NH3NH3
Balanced reaction is : 4 NH3 + 5 O2 4 NO + 6 H2O
Case 1 : Let NH3 be the limiting reagent
mass NH3 = 26 g
moles NH3 = (mass NH3) / (molar mass NH3)
moles NH3 = (26 g) / (17.0 g/mol)
moles NH3 = 1.53 mol
moles NO formed = moles NH3
moles NO formed = 1.53 mol
Case 2 : let O2 be the limiting reagent
mass O2 = 26 g
moles O2 = (mass O2) / (molar mass O2)
moles O2 = (26 g) / (32.0 g/mol)
moles O2 = 0.8125 mol
moles NO formed = (moles O2 consumed) * (4 moles NO / 5 moles O2)
moles NO formed = (0.8125 mol) * (4/5)
moles NO formed = (0.8125 mol) * (0.8)
moles NO formed = 0.650 mol
Since less moles of NO are formed in Case 2, therefore, O2 is the limiting reagent.
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