Final answer:
The question seems to contain an error, as magnesium chloride does not directly react with aluminum to form aluminum chloride. The given balanced equation involves aluminum reacting with chlorine gas, not magnesium chloride, to produce aluminum chloride. A direct calculation isn't possible without additional context or reaction pathways.
Step-by-step explanation:
To determine how many grams of aluminum chloride (AlCl3) would be produced from reacting 50.0 g of aluminum (Al) with 125g of magnesium chloride (MgCl2), we first need to establish the balanced equation for the reaction between aluminum and chlorine gas, since magnesium chloride doesn't react directly with aluminum to produce aluminum chloride. The relevant balanced equation is:
2 Al(s) + 3 Cl2(g) → 2 AlCl3(s)
However, to use this equation directly, we would need to convert magnesium chloride to chlorine gas. Since the question provides no further information or context to facilitate this conversion, there seems to be an error in the question. Typically, aluminum would react with chlorine gas, not magnesium chloride, to produce aluminum chloride. If we consider a hypothetical situation where magnesium chloride could react with aluminum to produce aluminum chloride, the reaction wouldn't be balanced as MgCl2 isn't a reactant for producing AlCl3.
Based on the provided balanced chemical equation, you would use stoichiometry to calculate the moles of AlCl3 produced from the given mass of Al. Then, using the molar mass of AlCl3, you could convert moles of AlCl3 to grams. However, the given situation with magnesium chloride doesn't align with the balanced equation, so a direct calculation isn't possible without additional context or reaction pathways.