led concentrated HCI solution in excess to 45. nd collected the hydrogen I gas that was prod Mg(s)+2HCl(aq)arrow MgCl_(2)(aq)+ collected 2.01 grams of H_(2) . what was the per answer to the nearest : tenth of a Type your answer in the boxes square square square

To determine the percent yield of the reaction, we need to follow these steps:1. Calculate the theoretical yield of hydrogen gas ( ).2. Calculate the percent yield using the actual yield and the theoretical yield.First, let's write down the balanced chemical equation for the reaction: From the balanced equation, we see that 1 mole of magnesium ( ) produces 1 mole of hydrogen gas ( ).Next, we need to find the molar mass of : Now, let's calculate the theoretical yield of . Given that we have 45 grams of , we first need to convert this mass to moles: Since the reaction is 1:1, the moles of produced will also be 1.85 moles. Now, we convert moles of to grams: Finally, we calculate the percent yield using the actual yield (2.01 grams) and the theoretical yield (3.72 grams): So, the percent yield of the reaction is approximately 53.8%.