The number of moles of Mg required to produce 11.212dm3 of Hydrogen at SIT when it reacts with HCl solution, are Mg + 2HCI MgCl2 + H2

Explanation

To find the number of moles of magnesium (Mg) required, consider the stoichiometry of the reaction: Mg + 2HCl → MgCl2 + H2. According to the ideal gas law, 1 mole of any gas at standard temperature and pressure (STP) occupies 22.4 dm3. Therefore, to produce 11.2 dm3 of hydrogen gas, 0.5 moles of Mg is required. Option C is correct. Option A suggests 1 mole of Mg, which would produce 22.4 dm3 of H2, double the required amount. Option B suggests 2 moles, producing an even larger volume of 44.8 dm3, and Option D suggests 0.25 moles, producing only 5.6 dm3 of H2, half of the required volume.