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)

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).

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