If 3.7 mols of Cl_(2) are used for this reaction how much HCl will be H_(2)(g)+Cl_(2)(g)arrow 2HCl(g) formed? Assume there are enough reactants to complete the reaction. 1.3 mols 3.7 mols 7.4 mols 9.3 mols

To determine how much HCl will be formed when 3.7 mols of Cl2 are used in the reaction, we need to use the stoichiometry of the balanced chemical equation.<br /><br />The balanced chemical equation for the reaction is:<br />H2(g) + Cl2(g) → 2HCl(g)<br /><br />From the equation, we can see that 1 mol of Cl2 reacts with 1 mol of H2 to produce 2 mols of HCl.<br /><br />Given that 3.7 mols of Cl2 are used, we can calculate the amount of HCl formed as follows:<br /><br />3.7 mols of Cl2 × (2 mols of HCl / 1 mol of Cl2) = 7.4 mols of HCl<br /><br />Therefore, the correct answer is 7.4 mols of HCl.