Final answer:
The limiting reactant in this reaction is magnesium metal.
Step-by-step explanation:
In order to determine the limiting reactant in a reaction, we need to compare the amount of each reactant to the stoichiometric ratio given by the balanced chemical equation. In this case, the balanced equation is: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
To find the limiting reactant, we need to convert the given quantities of magnesium and hydrochloric acid to moles. The molar mass of magnesium is 24.31 g/mol and the molar mass of hydrochloric acid is 36.46 g/mol. Converting 0.0350 g of magnesium to moles, we get: 0.0350 g / 24.31 g/mol = 0.00144 mol of magnesium. Converting 10.00 mL of 6 M hydrochloric acid to moles, we get: 10.00 mL * 0.006 mol/mL = 0.0600 mol of hydrochloric acid.
According to the balanced equation, the ratio of magnesium to hydrochloric acid is 1:2. This means that for every 1 mole of magnesium, 2 moles of hydrochloric acid are required. Since we have 0.00144 mol of magnesium and 0.0600 mol of hydrochloric acid, we can see that there is an excess of hydrochloric acid.
Therefore, the limiting reactant in this reaction is magnesium metal.