observing changes to equilibrium forestville central school regents chemistry
TRANSCRIPT
Observing Observing Changes to Changes to EquilibriumEquilibrium
Forestville Central SchoolForestville Central School
Regents ChemistryRegents Chemistry
IntroductionIntroduction In this experiment you will be introduced to In this experiment you will be introduced to
chemical equilibrium. chemical equilibrium. You will then be presented with a number of You will then be presented with a number of
systems at equilibrium and will be asked to systems at equilibrium and will be asked to "stress" these systems by changing the "stress" these systems by changing the concentration of one of the reactants or products concentration of one of the reactants or products or by changing the temperature of the system. or by changing the temperature of the system.
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ExperimentsExperiments Complete each one of the experiments below and Complete each one of the experiments below and
answer the questions on your worksheet. answer the questions on your worksheet. Click Click on the pictures to guide you.on the pictures to guide you.
Cobalt System
Ammonium System
Iron Thiocyanate System
Chromate System
Copper SulfateSystem
Cobalt SystemCobalt System
NOTES: - Silver ions react with chloride ions to form the insoluble compound silver chloride.
1)
2)
3)
4)
5) Hint: read the note belowCoCl4
2-
Hint: Think aboutThe Cl- ion
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Cobalt SystemCobalt System
1) Answer:1) Answer: Equilibrium shifts to the leftEquilibrium shifts to the left
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Cobalt SystemCobalt System
2) Answer:2) Answer: Equilibrium shifts to the rightEquilibrium shifts to the right
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Cobalt SystemCobalt System
3) Answer:3) Answer: Equilibrium shifts to the RightEquilibrium shifts to the Right
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Cobalt SystemCobalt System
4) Answer:4) Answer: Equilibrium shifts to the leftEquilibrium shifts to the left
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Cobalt SystemCobalt System
5) Answer:5) Answer: Equilibrium shifts to the right due to Equilibrium shifts to the right due to
the precipitation out of the Clthe precipitation out of the Cl-- ions in ions in AgCl.AgCl.
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Ammonium SystemAmmonium System
NOTES: - The purplish color is due to phenolphthalein. The darker the purple color, the larger the hydroxide ion concentration in solution.
1)
2)
pink Colorless
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Ammonium SystemAmmonium System
1) Answer:1) Answer: Equilibrium shifts to the right (see Equilibrium shifts to the right (see
notes regarding color)notes regarding color)
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Ammonium SystemAmmonium System
2) Answer:2) Answer: Increase in temperature shifts the Increase in temperature shifts the
equilibrium to the RIGHTequilibrium to the RIGHT
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Iron Thiocyanate Iron Thiocyanate
NOTES: - the HPO4-2 ion forms a complex with the Fe+3 ion.
1)
2)
3)
4)
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Hint: See notes
1) Answer:1) Answer: Equilibrium shifts to the RightEquilibrium shifts to the Right
Iron Thiocyanate Iron Thiocyanate
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2) Answer:2) Answer: Equilibrium shifts to the rightEquilibrium shifts to the right
Iron Thiocyanate Iron Thiocyanate
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3) Answer3) Answer Equilibrium shifts to the leftEquilibrium shifts to the left
Iron Thiocyanate Iron Thiocyanate
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4) Answer4) Answer Due to the removal of FeDue to the removal of Fe+3+3, equilibrium , equilibrium
shifts to the leftshifts to the left
Iron Thiocyanate Iron Thiocyanate
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Chromate SystemChromate System
Na2CrO4
1)
Na2Cr2O7
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2)
Chromate SystemChromate System
1) Answer:1) Answer: Equilibrium shifts to the rightEquilibrium shifts to the right
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Chromate SystemChromate System
2) Answer:2) Answer: Equilibrium shifts to the leftEquilibrium shifts to the left
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Copper Sulfate SystemCopper Sulfate System
Answer:Answer: Equilibrium shifts to the right as water Equilibrium shifts to the right as water
is heated offis heated off
Copper Sulfate SystemCopper Sulfate System
Question:What if you add water Back to the dish?
Copper Sulfate SystemCopper Sulfate System
Answer:Answer: Equilibrium shifts back to the left as Equilibrium shifts back to the left as
water is added back to the unhydrated water is added back to the unhydrated crystalcrystal
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