Question

1.50 g of magnesium metal is reacted in a vessel containing 1.25 g oxygen gas to produce sold magnesium oxide as the only product. calculate the total mass of mgo produced in this reaction

Answer 1

The total mass of MgO produced in the reaction is 2.49 g. We calculate the mass of MgO produced by multiplying the moles of MgO by its molar mass: Mass of MgO = moles of MgO * molar mass of MgO = 0.0617 mol * 40.31 g/mol = 2.49 g

Step-by-step explanation:

In this reaction, magnesium (Mg) reacts with oxygen (O2) to produce magnesium oxide (MgO). The balanced equation for this reaction is: 2Mg + O2 → 2MgO

To determine the total mass of MgO produced, we need to calculate the amount of Mg and O2 reacted. The molar mass of Mg is 24.31 g/mol, and the molar mass of O2 is 32.00 g/mol.

First, we calculate the moles of Mg and O2 using their respective masses and molar masses:

Moles of Mg = mass of Mg / molar mass of Mg = 1.50 g / 24.31 g/mol = 0.0617 mol

Moles of O2 = mass of O2 / molar mass of O2 = 1.25 g / 32.00 g/mol = 0.0391 mol

The balanced equation tells us that 2 moles of MgO are produced for every 2 moles of Mg and 1 mole of O2. Therefore, the moles of MgO produced is equal to the moles of Mg:

Moles of MgO = moles of Mg = 0.0617 mol

Finally, we calculate the mass of MgO produced by multiplying the moles of MgO by its molar mass:

Mass of MgO = moles of MgO * molar mass of MgO = 0.0617 mol * 40.31 g/mol = 2.49 g

Therefore, the total mass of MgO produced in this reaction is 2.49 g.