Diatomic o2 can react with the element magnesium to form magnesium oxide (mgo). the balanced chemical equation is: o2 + 2 mg → 2 mgo if 97.2 g grams of magnesium totally reacted with more than enough o2, how many moles of mgo would be expected to form?

We expected 4 moles of MgO to be formed. (This is 161.2 grams)

Explanation:

Step 1: The balanced equation

O2 + 2 Mg → 2 MgO

Step 2: Data given

mass of Mg = 97.2 grams

O2 = in excess

Molar mass of Mg = 24.3 g/mol

Molar mass of O2 = 32 g/mol

Molar mass of MgO = 40.3 g/mol

Step 3: Calculate moles of Mg

moles Mg = 97.2 / 24.3 g/mol

moles Mg = 4 moles

Mg is the limiting reactant. It will completely react (4 moles). O2 is in excess. There will react 2 moles of 02.

Step 4: Calculate moles of MgO

For 2 moles Mg consumed, we need 1 mole O2 to produce 2 moles of MgO

For 4 moles of Mg consumed,  we have 4 moles of MgO produced.

We expected 4 moles of MgO to be formed. (This is 161.2 grams)

in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume