4 05 Chemical Reactions
Name: Yaissa Fernandez 4.05: Chemical Reactions
Data and Observations:
Complete a data table that includes a prediction of reaction type, observations, and identification of reaction type for each reaction in the lab. (10 points)
Reactants
Prediction of Reaction type
Observations
Reaction Type
Iron (III) and Copper (II) Sulfate Solution
Single replacement
Solids stay concentrated at the bottom
Single replacement
Lead (II) Nitrate and Potassium Iodide Solutions
Double replacement
Yellow powder collected at bottom
Double replacement
Magnesium Metal Ribbon and Hydrochloric Acid Solution
Single replacement
Solution begins to fizz
Single replacement
Electrolysis of Water
Decomposition
Water bubble in the tubes of H2 and O2 decomposition Burning Magnesium combustion When in contact with the CO2, it makes a bright light synthesis Conclusion:
1. Write a balanced equation for each reaction observed in this lab. (10 points total, 2 points each)
Iron (III) and Copper (II) Sulfate Solution:
2Fe+3CuSO4=3Cu+Fe2 (SO3)3
Lead (II) Nitrate and Potassium Iodide Solutions:
Pb (NO3)2+2KI=PbI2+2K (NO3)
Magnesium Metal Ribbon and Hydrochloric Acid Solution:
Mg+2HCl=MgCl2+H2
Electrolysis of Water:
2H2O=2H2+O2
Burning Magnesium:
2Mg+O2=2MgO
2. If you were to measure the mass of magnesium and hydrochloric acid before combining them in the test tube, how would that mass compare to the mass of reactants left in the test tube after the reaction? Explain your answer and how it corresponds to the law of conservation of mass. (5 points)
It would be the same mass, because according to law of conservation of mass: Energy cannot be created nor destroyed, only changed. But, since this happened in an open test tube with a gaseous product, the mass would most likely be less after combining them than before combining them.
3. One of the reactions you conducted can actually be categorized as TWO different types of reactions. Which reaction is this, and what are the two types of reactions?
Data and Observations:
Complete a data table that includes a prediction of reaction type, observations, and identification of reaction type for each reaction in the lab. (10 points)
Reactants
Prediction of Reaction type
Observations
Reaction Type
Iron (III) and Copper (II) Sulfate Solution
Single replacement
Solids stay concentrated at the bottom
Single replacement
Lead (II) Nitrate and Potassium Iodide Solutions
Double replacement
Yellow powder collected at bottom
Double replacement
Magnesium Metal Ribbon and Hydrochloric Acid Solution
Single replacement
Solution begins to fizz
Single replacement
Electrolysis of Water
Decomposition
Water bubble in the tubes of H2 and O2 decomposition Burning Magnesium combustion When in contact with the CO2, it makes a bright light synthesis Conclusion:
1. Write a balanced equation for each reaction observed in this lab. (10 points total, 2 points each)
Iron (III) and Copper (II) Sulfate Solution:
2Fe+3CuSO4=3Cu+Fe2 (SO3)3
Lead (II) Nitrate and Potassium Iodide Solutions:
Pb (NO3)2+2KI=PbI2+2K (NO3)
Magnesium Metal Ribbon and Hydrochloric Acid Solution:
Mg+2HCl=MgCl2+H2
Electrolysis of Water:
2H2O=2H2+O2
Burning Magnesium:
2Mg+O2=2MgO
2. If you were to measure the mass of magnesium and hydrochloric acid before combining them in the test tube, how would that mass compare to the mass of reactants left in the test tube after the reaction? Explain your answer and how it corresponds to the law of conservation of mass. (5 points)
It would be the same mass, because according to law of conservation of mass: Energy cannot be created nor destroyed, only changed. But, since this happened in an open test tube with a gaseous product, the mass would most likely be less after combining them than before combining them.
3. One of the reactions you conducted can actually be categorized as TWO different types of reactions. Which reaction is this, and what are the two types of reactions?