Given the following, what is the limiting reactant? What is the theoretical yield of #Cl_2#? If the yield of the reaction is 75.5%, what is the actual yield of chlorine?
Chlorine gas can be prepared in the laboratory by the following reaction: #4HCl(aq) + MnO_2(s) -> MnCl_2(aq) + 2H_2O(l) + Cl_2(g)# . You add 40.5 g of #MnO_2# to a solution containing 41.7 g #HCl# .
Chlorine gas can be prepared in the laboratory by the following reaction:
1 Answer
The actual yield is 3.83 g of
Explanation:
This is a limiting reactant problem.
We know that we will need a balanced equation with masses, molar masses, and moles of the compounds involved.
1. Gather all the information in one place with molar masses above the formulas and everything else below the formulas.
2. Identify the limiting reactant
An easy way to identify the limiting reactant is to calculate the "moles of reaction" each will give:
You divide the moles of each reactant by its corresponding coefficient in the balanced equation.
I did that for you in the table above.
3. Calculate the theoretical moles of
4. Calculate the theoretical yield of
5. Calculate the actual yield
The actual yield of