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5. Generally, in order to do a stoichiometry problem, you need a complete balanced equation. However, in some cases it is possible to do some stoichiometric calculations without the complete equation as long as a particular element is present in only one reactant and one product. For example, if you were told that an experiment converted FeCl3 to Fe;O4 and that those were the only reactants and products that contained iron (Fe), you would know that there would have to be 3 moles of FeCl3 for every 1 mole of Fe;O4 or else the iron would not balance. You would not know for sure whether the balancing coefficients were actually 3 and 1 (They might be 6 and 2, 9 and 3, 12 and 4, etc) but you would know that they had to be in a 3 to 1 ratio and that would be enough to relate those two compounds with the correct stoichiometry. a) In Part I of your experiment, potassium carbonate (K2CO3) was the only reactant which contained carbon (C) and strontium carbonate (SICO3) was the only product containing carbon. Using the mass of STCO3 which you collected in Part I of the experiment, determine the volume of 1.16 M K2CO3 solution used in excess. Show all reasoning. b) Clearly explain why it was necessary in this experiment to use an excess of the potassium carbonate solution.

5. Generally, in order to do a stoichiometry problem, you need a complete balanced equation. However, in some cases it is possible to do some stoichiometric calculations without the complete equation as long as a particular element is present in only one reactant and one product. For example, if you were told that an experiment converted FeCl3 to Fe;O4 and that those were the only reactants and products that contained iron (Fe), you would know that there would have to be 3 moles of FeCl3 for every 1 mole of Fe;O4 or else the iron would not balance. You would not know for sure whether the balancing coefficients were actually 3 and 1 (They might be 6 and 2, 9 and 3, 12 and 4, etc) but you would know that they had to be in a 3 to 1 ratio and that would be enough to relate those two compounds with the correct stoichiometry. a) In Part I of your experiment, potassium carbonate (K2CO3) was the only reactant which contained carbon (C) and strontium carbonate (SICO3) was the only product containing carbon. Using the mass of STCO3 which you collected in Part I of the experiment, determine the volume of 1.16 M K2CO3 solution used in excess. Show all reasoning. b) Clearly explain why it was necessary in this experiment to use an excess of the potassium carbonate solution.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter3: Calculations With Chemical Formulas And Equaitons
Section: Chapter Questions
Problem 3.141QP: A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume...
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5. Generally, in order to do a stoichiometry problem, you need a complete balanced equation. However, in some cases it is possible to do some stoichiometric calculations without the complete equation as long as a particular element is present in only one reactant and one product. For example, if you were told that an experiment converted FeCl3 to Fe3O4 and that those were the only reactants and products that contained iron (Fe), you would know that there would have to be 3 moles of FeCl3 for every 1 mole of Fe;O4 or else the iron would not balance. You would not know for sure whether the balancing coefficients were actually 3 and 1 (They might be 6 and 2, 9 and 3, 12 and 4, etc) but you would know that they had to be in a 3 to 1 ratio and that would be enough to relate those two compounds with the correct stoichiometry. a) In Part I of your experiment, potassium carbonate (K,CO3) was the only reactant which contained carbon (C) and strontium carbonate (SrCO3) was the only product containing carbon. Using the mass of SRCO; which collected in Part I of the experiment, determine the volume of 1.16 M K2CO3 solution used in excess. Show all reasoning. b) Clearly explain why it was necessary in this experiment to use an excess you of the potassium carbonate solution.
Transcribed Image Text:5. Generally, in order to do a stoichiometry problem, you need a complete balanced equation. However, in some cases it is possible to do some stoichiometric calculations without the complete equation as long as a particular element is present in only one reactant and one product. For example, if you were told that an experiment converted FeCl3 to Fe3O4 and that those were the only reactants and products that contained iron (Fe), you would know that there would have to be 3 moles of FeCl3 for every 1 mole of Fe;O4 or else the iron would not balance. You would not know for sure whether the balancing coefficients were actually 3 and 1 (They might be 6 and 2, 9 and 3, 12 and 4, etc) but you would know that they had to be in a 3 to 1 ratio and that would be enough to relate those two compounds with the correct stoichiometry. a) In Part I of your experiment, potassium carbonate (K,CO3) was the only reactant which contained carbon (C) and strontium carbonate (SrCO3) was the only product containing carbon. Using the mass of SRCO; which collected in Part I of the experiment, determine the volume of 1.16 M K2CO3 solution used in excess. Show all reasoning. b) Clearly explain why it was necessary in this experiment to use an excess you of the potassium carbonate solution.
Data Table for Part I Mass of unknown used: 2.45g (. ११५ (629 Mass of dry filter paper and strontium carbonate (SRCO3): Mass of empty filter paper (after folding and tearing): 1.37 g 9. Mass of strontium carbonate obtained: Data Table for Part II 29.27 26.14g 3.13g 28.02g Mass of crucible, lid and unknown sample: Mass of empty crucible and lid: Mass of unknown sample used: Mass of crucible, lid and contents after first heating: 28.029 Mass of crucible, lid and contents after second heating: Mass of crucible, lid and contents after third heating (if necessary): Mass of crucible, lid and contents after fourth heating (if necessary): 28.029 26.149 Final mass of crucible, lid and contents after heating: Mass of empty crucible and lid (from above): 1.88.9 3.139 Mass of residue after water loss: Mass of original unknown (from above): Mass of water contained in unknown sample:
Transcribed Image Text:Data Table for Part I Mass of unknown used: 2.45g (. ११५ (629 Mass of dry filter paper and strontium carbonate (SRCO3): Mass of empty filter paper (after folding and tearing): 1.37 g 9. Mass of strontium carbonate obtained: Data Table for Part II 29.27 26.14g 3.13g 28.02g Mass of crucible, lid and unknown sample: Mass of empty crucible and lid: Mass of unknown sample used: Mass of crucible, lid and contents after first heating: 28.029 Mass of crucible, lid and contents after second heating: Mass of crucible, lid and contents after third heating (if necessary): Mass of crucible, lid and contents after fourth heating (if necessary): 28.029 26.149 Final mass of crucible, lid and contents after heating: Mass of empty crucible and lid (from above): 1.88.9 3.139 Mass of residue after water loss: Mass of original unknown (from above): Mass of water contained in unknown sample:
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