NaHCO3 (aq) + CH3COOH (aq) ----> CO2 (g) + H2O (l) + CH3COONa (aq)
What is the molar ratio of NaHCO3 to CH3COONa?
What is the molar mass of each of the reactants and products?
How many moles of H2O will be produced from 2 moles of CH3COOH?
how many grams of CH3COOH?
How many grams of CO2 is produced from 3.2 grams of NaHCO3?
In this lab you will measure out the required amount and perform the combine the ingredients in a ziploc bag. You will measure the mass of the bag with the entire contents before and after the reaction.
Does your experiment abide by the law of convervation of mass? Why or why not?
Sunday, December 5, 2010
Stoichiometry Review Problems
For the questions on this worksheet, consider the following equation:
Ca(OH)2(s) + 2 HCl(aq) ---> CaCl2(aq) + 2 H2O(l)
1) What type of chemical reaction is taking place? _____________________
2) How many liters of 0.100 M HCl would be required to react completely with 5.00 grams of calcium hydroxide?
3) If I combined 15.0 grams of calcium hydroxide with 75.0 mL of 0.500 M HCl, how many grams of calcium chloride would be formed?
4) What is the limiting reagent from the reaction in problem #3? __________
5) How many grams of the excess reagent will be left over after the reaction in problem 3 is complete?
Solve the following stoichiometry grams-grams problems:
1) Using the following equation:
2 NaOH + H2SO4 ---> 2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
2) Using the following equation:
Pb(SO4)2 + 4 LiNO3 ---> Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?
Percent Yield Practice
1) Write the equation for the reaction of iron (III) phosphate with sodium sulfate to make iron (III) sulfate and sodium phosphate.
2) If I perform this reaction with 25 grams of iron (III) phosphate and an excess of sodium sulfate, how many grams of iron (III) sulfate can I make?
3) If 18.5 grams of iron (III) sulfate are actually made when I do this reaction, what is my percent yield?
4) Is the answer from problem #3 reasonable? Explain.
5) If I do this reaction with 15 grams of sodium sulfate and get a 65.0% yield, how many grams of sodium phosphate will I make?
Ca(OH)2(s) + 2 HCl(aq) ---> CaCl2(aq) + 2 H2O(l)
1) What type of chemical reaction is taking place? _____________________
2) How many liters of 0.100 M HCl would be required to react completely with 5.00 grams of calcium hydroxide?
3) If I combined 15.0 grams of calcium hydroxide with 75.0 mL of 0.500 M HCl, how many grams of calcium chloride would be formed?
4) What is the limiting reagent from the reaction in problem #3? __________
5) How many grams of the excess reagent will be left over after the reaction in problem 3 is complete?
Solve the following stoichiometry grams-grams problems:
1) Using the following equation:
2 NaOH + H2SO4 ---> 2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
2) Using the following equation:
Pb(SO4)2 + 4 LiNO3 ---> Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?
Percent Yield Practice
1) Write the equation for the reaction of iron (III) phosphate with sodium sulfate to make iron (III) sulfate and sodium phosphate.
2) If I perform this reaction with 25 grams of iron (III) phosphate and an excess of sodium sulfate, how many grams of iron (III) sulfate can I make?
3) If 18.5 grams of iron (III) sulfate are actually made when I do this reaction, what is my percent yield?
4) Is the answer from problem #3 reasonable? Explain.
5) If I do this reaction with 15 grams of sodium sulfate and get a 65.0% yield, how many grams of sodium phosphate will I make?
Bellringer 5
Using the equation below, calcuate the following:
Molar ratio
Molar mass
Mole to mole (given 2 moles of HBr)
Mole to gram (given 43 grams of HBr)
Gram to Percent Yield
HBr + ___ KHCO3 --->___ H2O + ___ KBr + ___ CO2
Molar ratio
Molar mass
Mole to mole (given 2 moles of HBr)
Mole to gram (given 43 grams of HBr)
Gram to Percent Yield
HBr + ___ KHCO3 --->___ H2O + ___ KBr + ___ CO2
Stoichiometry Tutoring Link
go to this link to assist you with solving stoichiometry problems.
http://www.chemtutor.com/mols.htm
http://www.chemtutor.com/mols.htm
More Stoichiometry
1a) How many moles of chlorine gas (Cl2) would react with 5 moles of sodium (Na) according
to the following chemical equation? (Balance equation.)
Na + Cl2 --> NaCl
1b) Using the equation (after it is balanced) above, determine the amount of product that can be
produced from 24.7 g Na.
1c) How many molecules of product would be produced from 24.7g Na?
__________________________________________________________________________________
2a) In the reaction 2C8H18 + 25O2 --> 16CO2 + 18 H2O, the ratio of volumes of O2 to CO2
is _________________.
2b) If 27.3g of C8H18 are combusted, what mass of water will be produced?
2c) How many molecules of CO2 will be produced?
2d) How many atoms of H are in 2 mol of C8H18?
2e) What is the percentage, by mass, of the H in 2 mol of C8H18?
to the following chemical equation? (Balance equation.)
Na + Cl2 --> NaCl
1b) Using the equation (after it is balanced) above, determine the amount of product that can be
produced from 24.7 g Na.
1c) How many molecules of product would be produced from 24.7g Na?
__________________________________________________________________________________
2a) In the reaction 2C8H18 + 25O2 --> 16CO2 + 18 H2O, the ratio of volumes of O2 to CO2
is _________________.
2b) If 27.3g of C8H18 are combusted, what mass of water will be produced?
2c) How many molecules of CO2 will be produced?
2d) How many atoms of H are in 2 mol of C8H18?
2e) What is the percentage, by mass, of the H in 2 mol of C8H18?
Homework 1
Balance the following equations:
1) ___ N2 + ___ F2 ___ NF3
2) ___ C6H10 + ___ O2 ___ CO2 + ___ H2O
3) ___ HBr + ___ KHCO3 ___ H2O + ___ KBr + ___ CO2
4) ___ GaBr3 + ___ Na2SO3 ___ Ga2(SO3)3 + ___ NaBr
5) ___ SnO + ___ NF3 ___ SnF2 + ___ N2O3
Using the equation from problem 2 above, answer the following questions:
6) If I do this reaction with 35 grams of C6H10 and 45 grams of oxygen, how many grams of carbon dioxide will be formed?
7) What is the limiting reagent for problem 6? ___________
8) How much of the excess reagent is left over after the reaction from problem 6 is finished?
9) If 35 grams of carbon dioxide are actually formed from the reaction in problem 6, what is the percent yield of this reaction?
1) ___ N2 + ___ F2 ___ NF3
2) ___ C6H10 + ___ O2 ___ CO2 + ___ H2O
3) ___ HBr + ___ KHCO3 ___ H2O + ___ KBr + ___ CO2
4) ___ GaBr3 + ___ Na2SO3 ___ Ga2(SO3)3 + ___ NaBr
5) ___ SnO + ___ NF3 ___ SnF2 + ___ N2O3
Using the equation from problem 2 above, answer the following questions:
6) If I do this reaction with 35 grams of C6H10 and 45 grams of oxygen, how many grams of carbon dioxide will be formed?
7) What is the limiting reagent for problem 6? ___________
8) How much of the excess reagent is left over after the reaction from problem 6 is finished?
9) If 35 grams of carbon dioxide are actually formed from the reaction in problem 6, what is the percent yield of this reaction?
Bellringer 4
Calculate the number of grams of NaCl produced as a result of 62.4 gram of sodium reacting with chlorine. The balance equation is :
Na + Cl ---> NaCl
Na + Cl ---> NaCl
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