Materials
• 250 mL filter flask
• Rubber stopper
• 2 rubber tubings
• Water trough
• 4-5 glass bottles
• 4-5 glass plates
• 10 mL Ammonia 3M
• 4-5 mL Copper Sulfate 0.2M
• Hydrogen Peroxide
• Wooden splint
• Sulfur
• Charcoal
• Steel Wool
• Copper Powder
• Selenium Powder
Methods
1) Make oxygen filled glass bottles
Transfer 10mL of CuSO4 into a flask
Add ammonium into the flask
Set up water trough, fill it 3/4 full with water
Fill glass bottles with water
Invert the glass bottles in the water trough
Slowly pour hydrogen peroxide to collect gas in the bottles
Remove glass bottles containing oxygen gas
2) In the fume hood, burn the solids over a Bunsen burner. Observe the flame color
3) Put the burning solids into the oxygen bottles. Observe the flame color.
Data&Results
Conclusion
The hypothesis that the solids burn with a red flame is false. Not all solids burned with a red flame. For example the selenium powder burned with a blue flame over the Bunsen burner and with an even brighter blue flame in the oxygen bottle.
The hypothesis that all solids burn more brightly in an atmosphere of pure oxygen is true. All the solids burned more brightly in the oxygen bottles than over the Bunsen burner.
Hypothesis
1)All solids will burn with a red flame
2)All solids burn more brightly in an atmosphere of pure oxygen than they do in air
Oxygen, Oxygen, Oxygen --> What a Flame!
By Winnie Wu, Jenifer Criollo, Jessica Alvarez, Nadia Alkaysey
Observations
Discussion
sulfur
The solids burned with orange, blue and green flames over the Bunsen Burner. When burned in the oxygen bottles, the flames were noticeably brighter(bright orange, bright blue, bright green)
Imagine that you are given two metal oxides to stud in the lab. You heat each oxide in a small test tube and then insert a glowing splint in each. You observe that the splint in tube 1 immediately ignites and burns with a steady flame before it dies but the splint in tube 2 does not.
What happened to the metal oxide in tube 1 when it was heated?
Do both metal oxides decompose when heated?
What can you conclude about the stability of the 2 oxides based on these observations?
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