Magnesium can be used as a 'getter' in evacuated enclosuresto react with the last traces of oxygen. (The magnesium isusually heated by passing an electric current through a wireor ribbon of the metal.) If an enclosure of 5.67 L has a partialpressure of O2 of 7.066 mPa at 30 °C, what mass of magnesiumwill react according to the following equation?2 Mg1s2 + O21g2¡2 MgO1s2

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amount of a substance needed or produced in a reaction. In this case, the stoichiometric coefficients from the equation 2 Mg + O2 → 2 MgO indicate that two moles of magnesium react with one mole of oxygen, which is essential for calculating the mass of magnesium required.

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is crucial for determining the number of moles of oxygen present in the enclosure at the given conditions. By using the partial pressure of O2 and the volume of the enclosure, we can calculate the moles of oxygen available for the reaction with magnesium.

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between moles and grams when calculating the mass of magnesium needed for the reaction. For magnesium, the molar mass is approximately 24.31 g/mol, which will be used to find the total mass of magnesium that reacts with the calculated moles of oxygen.