10.0 g of NO and 10.0 g of O2 react together in the following unbalancedd reaction. How many grams of NO2 will be formed?
NO + O2 --> NO2
The balanced equation is
2 NO + O2 -----> 2 NO2
Number of moles of NO = 10.0 g / 30.01 g/mol = 0.333 mole
Number of moles of O2 = 10.0 g / 32.0 g/mol = 0.313 mole
From the balanced equation we can say that
2 mole of NO requires 1 mole of O2 so
0.333 mole of NO will require
= 0.333 mole of NO *(1 mole of O2 / 2 mole of NO)
= 0.157 mole of O2
But we have 0.313 mole of O2 which is in excess so O2 is an excess reactant and NO is limiting reactant
From the balanced equation we can say that
2 mole of NO produces 2 mole of NO2 so
0.333 mole of NO will produce
= 0.333 mole of NO *(2 mole of NO2 / 2 mole of NO)
= 0.333 mole of NO2
mass of 1 mole of NO2 = 46.0055 g so
the mass of 0.333 mole of NO2 = 15.3 g
Therefore, the mass of NO2 produced would be 15.3 g
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