C.4.5 Use a balanced chemical equation to calculate the quantities of reactants needed and products made in a chemical reaction that goes to completion.
Learning Goals:
I can use a balanced chemical equation to calculate the quantities of reactants needed in a completed chemical reaction.
I can use a balanced chemical equation to calculate the products made in a completed chemical reaction.
C.4.5 Use a balanced chemical equation to calculate the quantities of reactants needed and products made in a chemical reaction that goes to completion.
Learning Goals:
I can use a balanced chemical equation to calculate the quantities of reactants needed in a completed chemical reaction.
I can use a balanced chemical equation to calculate the products made in a completed chemical reaction.
You Need:
Scientific Calculator (recommend - Natural Scientific Calculator app for cellphone)
Paper
Pencil (it erases...)
Periodic Table (provided on each question).
The following reaction was performed:
LiOH + KCl → LiCl + KOH
20.0 g of LiOH was reacted with an excess of KCl to produce 6.0 g LiCl.
Step 1 - Balance the equation (if you need "1" of anything, place an _ in the blank - "shift" + "hyphen").
Step 2 - Calculate the theoretical yield of LiCl.
Theoretical yield
Step 3 - Calculate the percent yield if 6.0 g of LiCl was actually produced.
Percent yield
The following reaction was performed:
C3H8 + O2 → CO2 + H2O
5.0 g C3H8 is reacted with excess O2
Step 1 - Balance the equation (if you need "1" of anything, place an _ in the blank - "shift" + "hyphen").
Step 2 - Calculate the theoretical yield of H2O.
Theoretical yield
Step 3 - Calculate the percent yield if 7.9 g of H2O was actually produced.
Percent yield
The following reaction was performed:
NaCl + CaO → CaCl2 + Na2O
20.0 g of CaO is reacted with excess NaCl.
Step 1 - Balance the equation (if you need "1" of anything, place an _ in the blank - "shift" + "hyphen").
Step 2 - Calculate the theoretical yield of Na2O.
Theoretical yield
Step 3 - Calculate the percent yield if 4.5 g Na2O was produced.
Percent yield
The following reaction was performed:
Sn3(PO4)4 + Na2CO3 → Sn(CO3)2 + Na3PO4
36 grams Sn3(PO4)4 is reacted with an excess of Na2CO3
Step 1 - Balance the equation (if you need "1" of anything, place an _ in the blank - "shift" + "hyphen").
Step 2 - Calculate the theoretical yield of Sn(CO3)2
Theoretical Yield of Sn(CO3)2
Step 3 - Percent yield, if 29.8 g Sn(CO3)2 are actually produced.
Percent yield
The following reaction was performed:
H2 + N2 → NH3
5.0 grams N2 and 5.0 grams H2 were reacted to form 3.25 g of ammonia.
Step 1 - Balance the equation (if you need "1" of an anything, place an _ in the blank - "shift" + "hyphen").
Step 2 - Determine the mass of the product produced by each reactant.
For H2
For N2
Step 3 - Compare the amounts calculated in step 2 to identify the limiting reagent.
Limiting Reagent
Step 4 - The lowest quantity calculated in step 2 will be the theoretical yield.
Theoretical Yield
Step 5 - Calculate the percent yield if the actual product produced was measured to be 3.25g.
Percent yield
