Assume that you start with 2 mole(s) of magnesium metal, determine:
The number of grams of MgO(s) that would be produced in the following reaction (enter your answer with 4 significant figures):
Mg(s) + 1/2O2(g) → MgO(s)
2 mols Mg will produce 2 mols MgO.
2 mols MgO x molar mass MgO = grams MgO
80.62
To determine the number of grams of MgO(s) that would be produced in the reaction, you need to use stoichiometry to convert moles of magnesium (Mg) to moles of magnesium oxide (MgO), and then convert moles of MgO to grams.
Let's start by writing the balanced equation for the reaction:
Mg(s) + 1/2O₂(g) → MgO(s)
According to the balanced equation, 1 mole of Mg reacts with 1/2 mole of O₂ to produce 1 mole of MgO.
Given that you start with 2 moles of Mg, you can determine the number of moles of MgO produced using the stoichiometric ratio:
Moles of MgO = Moles of Mg * (1 mole of MgO / 1 mole of Mg)
Moles of MgO = 2 moles of Mg * (1 mole of MgO / 1 mole of Mg)
Moles of MgO = 2 moles of MgO
So, 2 moles of Mg will produce 2 moles of MgO.
Now, we need to convert moles of MgO to grams. To do this, we need to know the molar mass of MgO, which is calculated as:
Molar mass of MgO = Atomic mass of Mg + Atomic mass of O
Looking up the atomic masses of Mg and O from the periodic table, we find:
Molar mass of Mg = 24.305 g/mol
Molar mass of O = 15.999 g/mol
Molar mass of MgO = 24.305 g/mol + 15.999 g/mol
Molar mass of MgO ≈ 40.304 g/mol (rounded to four significant figures)
Now we can convert moles of MgO to grams:
Grams of MgO = Moles of MgO * Molar mass of MgO
Grams of MgO = 2 moles of MgO * 40.304 g/mol
Grams of MgO ≈ 80.608 g (rounded to four significant figures)
Therefore, the number of grams of MgO(s) produced in the reaction is approximately 80.608 g.