You may want to reference (Page) section 4.3 while completing this problem. Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is 2Mg(s)+O2(g)→2MgO(s) 2 M g ( s ) + O 2 ( g ) → 2 M g O ( s ) When 10.0 g g Mg M g is allowed to react with 10.6 g g O2 O 2 , 12.1 g g MgO Mg O is collected.

This is an incomplet question, here is a complete question.

Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is

When 10.0 g Mg is allowed to react with 10.6 g O₂, 12.1 g MgO is collected.

Determine the theoretical yield for the reaction.

Answer : The theoretical yield for the reaction is, 16.66 grams

Explanation : Given,

Mass of Mg = 10 g

Mass of = 10.6 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, 2 mole of react with 1 mole of

So, 0.4167 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, 2 mole of react to give 2 mole of

So, 0.4167 mole of react to give 0.4165 mole of

Now we have to calculate the mass of

Thus, the theoretical yield for the reaction is, 16.66 grams

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.