You run an experiment according to this equation: 2HCl+CaCO_(3)-gt H_(2)O+CaCl_(2) +CO_(2) When running your lab you started with 62 .16 grams of HCI and 50.18 grams of CaCO_(3) If, after the reaction finishes, your products have a total mass of 80.10, what was the percent yield? Round your answer to the nearest 0.01 and include units! Your Answer: square square Answer units

## Step 1: Calculate the molar masses of reactants and products### The molar mass of is , and the molar mass of is . These values will be used to determine the limiting reactant and theoretical yield.## Step 2: Determine moles of each reactant### Moles of . Moles of .## Step 3: Identify the limiting reactant### From the balanced equation, reacts with . Therefore, the required moles of for is . Since is available, is the limiting reactant.## Step 4: Calculate the theoretical yield of products### The total mass of products equals the mass of reactants due to the law of conservation of mass. Thus, the theoretical yield is the sum of the masses of and : Theoretical yield = .## Step 5: Calculate the percent yield### Percent yield is given by . Substituting the values: .