What mass of Ag2CO3(s) in grams is theoretically produced by mixing 125 mL of 0.315 M Na2CO3(aq) and 75.0 mL of 0.155 M AgNO3(aq)?
1.
What is the balanced equation for this reaction?
2. If you know the moles of sodium carbonate involved in the reaction, how can you determine the moles of silver carbonate that are produced?
3. How many moles of silver nitrate are available?
4. How many moles of silver carbonate can be made from the moles of silver nitrate available?
5. How many moles of silver carbonate can be made from 125 mL of 0.315 M sodium carbonate?
6. Comparing your answers to questions 4 and 5 above, how many moles of silver carbonate would actually be made from the reaction conditions in the model?
7. What term is applied to the reactant that produces the actual amount of product?
8. What is the theoretical yield of silver carbonate in grams?
9. Looking back over your answers to the previous questions, how could you calculate the grams of silver carbonate produced by setting up and solving only two equations?
Part 1
The balanced reaction
2AgNO3(aq) + Na2CO3(aq) =Ag2CO3(s) + 2NaNO3(aq)
Part 2
Moles of Na2CO3 = molarity x volume
= 0.315 mol/L x 125 mL x 1L/1000 mL
= 0.039375 mol
Moles of Ag2CO3 formed = 0.039375 mol
Part 3
Moles of AgNO3 = molarity x volume
= 0.155 mol/L x 75 mL x 1L/1000 mL
= 0.011625 mol
Part 4
Moles of Ag2CO3 formed =
= 1 mol Ag2CO3 x 0.011625 mol AgNO3 / 2 mol AgNO3
= 0.0058125 mol Ag2CO3
Part 5
From the stoichiometry of the reaction
2 mol of AgNO3 reacts with = 1 mol of Na2CO3
0.011625 mol of AgNO3 reacts with = 1* 0.011625/2
= 0.0058125 mol of Na2CO3
But we have more than required moles of Na2CO3
Excess reactant = Na2CO3
Limiting reactant = AgNO3
Moles of Ag2CO3 formed
= 1 mol Ag2CO3 x 0.011625 mol AgNO3 / 2 mol AgNO3
= 0.0058125 mol Ag2CO3
Mass of Ag2CO3 formed = Moles x molecular weight
= 0.0058125 mol x 275.75 g/mol
= 1.603 g
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