1.0 g of magnesium is burnt with 0.56


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1.0g of magnesium is burnt with 0.56g O2(oxygen) in a closed vessel . Which reactant is left in excess and how much ? (At. wt. Mg = 24 ; O = 16)

Answered by admin @



The equation is as follows:

2Mg + O2  ------>  2MgO
(s)      (g)                (s)

Therefore 2 moles of Mg require 1 mole of O2 to produce 2 moles of MgO.

Calculate actual moles.
moles= mass/ molar mass

Mg=    1/24  = 0.041667
O2=   0.56/32 = 0.0175
MgO=

Mole ratio of Mg: O2   = 2:1

find mass of Mg that reacts:

that means 2 mole of Mg reacts with 1 moles of O2

If 1 = 2 
Then 0.0175 = 0.0175 x 2
                     =0.035 moles of magnesium

mass of magnesium that reacts:

mass= moles x molar mass
        = 24 x 0.035
         
              0.84 g
That means that of the 1 gram of magnesium that reacts only 0.84 grams is used

Therefore magnesium is in excess and by 0.16

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