Final answer:
The mass of magnesium bromide formed when 1.0 g of magnesium reacts with 5.0 g of bromine is 5.0 g.
Step-by-step explanation:
In order to determine the mass of magnesium bromide formed when 1.0 g of magnesium reacts with 5.0 g of bromine, we need to identify the limiting reactant. To do this, we need to calculate the number of moles of each reactant. From the given information, 1.0 g of magnesium is equivalent to 0.0417 moles of magnesium, and 5.0 g of bromine is equivalent to 0.156 moles of bromine.
According to the balanced chemical equation for the reaction between magnesium and bromine, 1 mole of magnesium reacts with 2 moles of bromine to form 1 mole of magnesium bromide. Therefore, we can determine the theoretical yield of magnesium bromide by multiplying the number of moles of magnesium by the molar mass of magnesium bromide (184.11 g/mol).
The theoretical yield of magnesium bromide from the given amount of magnesium is 7.66 g. However, we have 5.0 g of bromine, which is less than the theoretical yield. This means that bromine is the limiting reactant, and the mass of magnesium bromide formed will be determined by the amount of bromine available, which is 5.0 g. Therefore, the answer is option D) 5.0 g.