Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. the balanced equation for the reaction is 2 mg(s) + o2(g) → 2 mgo(s) now consider that you react 10.0 g mg with 6.00 g o2 gas. if you were able to collect 9.62 g of mgo, what would be your percent yield for the reaction?

Answer : The percent yield of is, 64.13 %

Solution : Given,

Mass of Mg  = 10 g

Mass of = 6 g

Molar mass of Mg = 24 g/mole

Molar mass of = 32 g/mole

Molar mass of MgO = 40 g/mole

First we have to calculate the moles of Mg and .

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

From the balanced reaction we conclude that

As, 1 mole of react with 2 mole of

So, 0.1875 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of

From the reaction, we conclude that

As, 1 mole of react to give 2 mole of

So, 0.1875 moles of react to give moles of

Now we have to calculate the mass of

Theoretical yield of = 15 g

Experimental yield of = 9.62 g

Now we have to calculate the percent yield of

Therefore, the percent yield of is, 64.13 %

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.