14. Methanol, CH_(2)OH can be produced by the following reaction .Assume H_(2) is the limiting reactant and 4 mol of H_(2) are used in the reaction. If 1 mol of CH_(3)OH is produced by the reaction, what is the percent yield? 2H_(2)+COarrow CH_(3)OH Actual yield __ PercentYield= Theoretical yield __

To calculate the percent yield, we need to determine the theoretical yield and the actual yield.Given information:- The balanced chemical equation is: - 4 mol of are used in the reaction.- 1 mol of is produced by the reaction.Step 1: Calculate the theoretical yield.The theoretical yield is the maximum amount of product that can be formed from the given amount of reactants, assuming 100% efficiency.From the balanced equation, we can see that 2 mol of are required to produce 1 mol of .Theoretical yield = (1 mol ) × (2 mol / 1 mol ) = 2 mol Step 2: Calculate the actual yield.The actual yield is the amount of product that is actually formed in the reaction.Given that 1 mol of is produced by the reaction, the actual yield is 1 mol.Step 3: Calculate the percent yield.Percent yield = (Actual yield / Theoretical yield) × 100%Percent yield = (1 mol / 2 mol) × 100% = 50%Therefore, the percent yield of the reaction is 50%.