Reactions in Our World Lab Report


Reactions in Our World Lab Report

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Instructions: In this laboratory activity, you will be comparing chemical reactions to nuclear reactions by observing chemical phenomena in action. To prepare for your observations and data collection, you must complete the pre-lab activity worksheet that goes with this lab. Otherwise, you will not have the chemical equations you need to match each chemical reaction. Fill in each section of this lab report and submit it to your instructor for grading.

Title: Reactions in Our World

Objective(s): compare chemical reactions to nuclear reactions by observing chemical phenomena in actions

Hypothesis:

You will complete your hypotheses using the chart below and the balanced equations from your pre-lab activity. In each row, predict the reaction type/s for each chemical reaction. Reaction type options are synthesis, decomposition, single displacement, double displacement, acid-base reaction, combustion, and oxidation-reduction. Some reactions can fit more than one type of reaction.

Chemical Reaction

Prediction of Reaction Type

Iron and copper (II) sulfate solution

I predict the reaction between __Iron___ and ___copper sulfate__ will yield a ____single displacement______ reaction/s.

Lead (II) nitrate and potassium iodide solutions

I predict the reaction between ______ will yield a ___single displacement_______ reaction/s.

Magnesium metal and hydrochloric acid solution

I predict the reaction between _____ and ___hydrochloric acid__ will yield a __single displacement_____ reaction/s.

Electrolysis of water

I predict the reaction between _______ will yield a __oxidation reduction________ reaction/s.

Burning magnesium

I predict the reaction between __magnesium___ and __heat___ will yield a ___synthesis_______ reaction/s.

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.

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.

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.

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.

5. Burning magnesium

Place magnesium ribbon in a clean crucible (on a clay triangle above a Bunsen burner). Heat until the magnesium begins to burn.

Variables:

List your controlled variables, independent variable, and dependent variable for each experiment in the chart below.

Chemical Reaction

Controlled Variables

Independent Variable

Dependent Variable

Iron and copper (II) sulfate solution

Iron

Iron

copper

Lead (II) nitrate and potassium iodide solutions

lead nitrate

lead nitrate

potassium iodide

Magnesium metal and hydrochloric acid solution

magnesium metal

magnesium metal

hydrochloric acid

Electrolysis of water

hydrogen

hydrogen

oxygen

Burning magnesium

heat

heat

magnesium

Data and Observations:

Complete a data table that includes a prediction of reaction type (single replacement, double replacement, synthesis, decomposition, acid-base, oxidation-reduction, or combustion), observations, and identification of reaction type for each reaction in the lab.

Chemical Reaction

Observations

Reaction Type

Iron and copper (II) sulfate solution

the iron turned a brownish red color

Single Displacement

Lead (II) nitrate and potassium iodide solutions

It went toward the bottom of the test tube, and the solution appeared as a thick opaque yellow

Double Displacement

Magnesium metal and hydrochloric acid solution

Magnesium had bubbles forming around it, as if it were dissolving

Single Displacement

Electrolysis of water

Small bubbles began to form

Decomposition

Burning magnesium

the Magnesium produced red and white flames when heated

Synthesis

Analysis and Conclusion:

1. 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. 

2. Some of the reactions you conducted can be categorized as more than one type of reaction. Which reactions are these, and what are the types of reactions? 

3. Analyze your observations of each reaction. Based on the products made, were your predictions of chemical reaction type correct? In what other ways could you test your predictions to confirm their accuracy? 

4. How do the chemical reactions in this lab activity compare to nuclear reactions, such as fission and fusion? 


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