Question

What mass of Ag2CO3(s) in grams is theoretically produced by mixing 125 mL of 0.315 M...

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?

Homework Answers

Answer #1

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

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1) How many grams of Ag2CO3 will precipitate when excess K2CO3 solution is added to 53.0...
1) How many grams of Ag2CO3 will precipitate when excess K2CO3 solution is added to 53.0 mL of 0.713 M AgNO3 solution? 2AgNO3(aq) + K2CO3(aq) = Ag2CO3(s) + 2KNO3(aq) ?g 2)How many mL of 0.695 M HBr are needed to dissolve 8.81 g of MgCO3? 2HBr(aq) + MgCO3(s) = MgBr2(aq) + H2O(l) + CO2(g) ? mL
What is the maximum mass (in grams) of silver chloride that can be precipitated by mixing...
What is the maximum mass (in grams) of silver chloride that can be precipitated by mixing 50.0 mL of 0.025 M silver nitrate solution with 100.0 mL of 0.025 M sodium chloride solution? b.) Which reagent is in excess? c.) What is the concentration of chloride remaining in solution after the reaction has gone to completion?
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl,...
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl, how many extra mLs of excess reactant were used? AgNO3 (aq) + NH4Cl(aq) → AgCl(s) + NH4NO3 (aq)
How many grams of magnesium nitrate can be produced from 50.0 mL of a 2.0 mol/L...
How many grams of magnesium nitrate can be produced from 50.0 mL of a 2.0 mol/L nitric acid solution reacting with excess magnesium carbonate?
How many grams of Ni(OH)2 are produced from the reaction of 30.5 mL of 1.87 M...
How many grams of Ni(OH)2 are produced from the reaction of 30.5 mL of 1.87 M NaOH? NiCl2(aq)+2NaOH(aq)→Ni(OH)2(s)+2NaCl(aq)
How many grams of AgCl are produced from the reation of 135 mL of 0.567 M...
How many grams of AgCl are produced from the reation of 135 mL of 0.567 M AgNO3 with an excess of AlCl3
A) How many grams of solid silver nitrate would you need to prepare 150.0 mL of...
A) How many grams of solid silver nitrate would you need to prepare 150.0 mL of a 0.140 M AgNO3 solution? B) An experiment calls for you to use 100 mL of 0.30 M HNO3 solution. All you have available is a bottle of 3.8 M HNO3. How many milliliters of the 3.8 M HNO3 solution do you need to prepare the desired solution? C) How many milliliters of water do you need to prepare the desired solution?
How many grams of H2(g) can theoretically be produced from a 5-g sample of magnesium metal...
How many grams of H2(g) can theoretically be produced from a 5-g sample of magnesium metal and excess HCl(aq)?
How many grans of lithium nitrate will be formed from 50.0 mL of 2 M lithium...
How many grans of lithium nitrate will be formed from 50.0 mL of 2 M lithium bromide? What is the molarity of a silver nitrate solution if the reaction of 200 mL of silver nitrate solution with an excess of lithium bromine produces 1.3 moles of silver bromide?
A. You wish to prepare 198 grams of 10.3 % Na3PO4. How many grams will need...
A. You wish to prepare 198 grams of 10.3 % Na3PO4. How many grams will need of sodium phosphate and how many mL of water? Assume that the density of water is 1.00 g / ml. B. If 20.5 grams of an aqueous solution of cobalt(II) sulfate, CoSO4, contains 2.84 grams of cobalt(II) sulfate, what is the percentage by mass of cobalt(II) sulfate in the solution? C. An aqueous solution of lead nitrate, Pb(NO3)2, contains 8.74 grams of lead nitrate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT