Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction.2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)

Sure, here are the steps to solve this problem:

Step 1: Determine the number of moles of HCl from its molarity and volume. Molarity = moles/volume So, moles of HCl = Molarity * Volume = 0.743 mol/L * 0.250 L = 0.18575 mol

Step 2: Determine the number of moles of Fe from the given number of atoms using Avogadro's number. Number of moles = Number of atoms / Avogadro's number = 3.41 × 10^23 atoms / 6.022 × 10^23 atoms/mol = 0.566 mol

Step 3: From the balanced chemical equation, we can see that the mole ratio of HCl to Fe to H2 is 2:1:1. This means that for every mole of Fe, one mole of H2 is produced.

Step 4: Determine the limiting reactant, which is the reactant that will be completely consumed first and thus determines the maximum amount of product that can be formed. In this case, since we have less moles of HCl (0.18575 mol) than Fe (0.566 mol) and the mole ratio is 2:1, HCl is the limiting reactant.

Step 5: Determine the number of moles of H2 that can be formed from the limiting reactant. Since the mole ratio of HCl to H2 is 2:1, the number of moles of H2 that can be formed is half the number of moles of HCl. Moles of H2 = 0.18575 mol HCl * (1 mol H2 / 2 mol HCl) = 0.092875 mol H2

Step 6: Convert the number of moles of H2 to grams using its molar mass (2.02 g/mol). Mass of H2 = Moles of H2 * Molar mass of H2 = 0.092875 mol * 2.02 g/mol = 0.1875 g

So, 0.1875 grams of H2 can be formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 10^23 atoms of Fe.