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Procedure:
1. Iron (III) and copper (II) sulfate solution
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.
The Iron shavings change from dark gray to brown when it mixes with copper that changes from transparent to blue.
2. Lead (II) nitrate and potassium iodide solutions
Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction.
Lead nitrate and potassium are both transparent but when they mix t changes to a yellow color.
3. Magnesium metal and hydrochloric acid solution
Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next, place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas.
When magnesium and hydrochloric acid are mixed it starts boiling.
4. Electrolysis of water
Use a U-tube with electrodes at each end, connected to a battery. Fill the U-tube with water. Turning on the battery, observe the results at each electrode. Next, test for hydrogen and oxygen gas produced at each end of the tube.
When you turn on the battery, bubbling happens.
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 and copper Copper will probably melt It mixed Combustion Lead and nitrate Lead will probably melt It mixed Synthesis Magnesium metal and Hydrochloric Metal will probably melt Didn’t melt Acid Electrolysis of water Water will probably boil Boiled Decomposition Burning magnesium Magnesium will probably melt Didn’t melt Double displacement
Conclusion:
1. Write a balanced equation for each reaction observed in this
1. Iron (III) and copper (II) sulfate solution
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.
The Iron shavings change from dark gray to brown when it mixes with copper that changes from transparent to blue.
2. Lead (II) nitrate and potassium iodide solutions
Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction.
Lead nitrate and potassium are both transparent but when they mix t changes to a yellow color.
3. Magnesium metal and hydrochloric acid solution
Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next, place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas.
When magnesium and hydrochloric acid are mixed it starts boiling.
4. Electrolysis of water
Use a U-tube with electrodes at each end, connected to a battery. Fill the U-tube with water. Turning on the battery, observe the results at each electrode. Next, test for hydrogen and oxygen gas produced at each end of the tube.
When you turn on the battery, bubbling happens.
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 and copper Copper will probably melt It mixed Combustion Lead and nitrate Lead will probably melt It mixed Synthesis Magnesium metal and Hydrochloric Metal will probably melt Didn’t melt Acid Electrolysis of water Water will probably boil Boiled Decomposition Burning magnesium Magnesium will probably melt Didn’t melt Double displacement
Conclusion:
1. Write a balanced equation for each reaction observed in this