Oxidation-Reduction Reactions Temperature and Color Change Data for Oxidation of
ID: 1081291 • Letter: O
Question
Oxidation-Reduction Reactions
Temperature and Color Change Data for Oxidation of Iron
Time (s)
Temperature (oC)
Color observations
0
25°C
Brown
10
25.8 °C
Amber
20
26.6°C
Amber
30
28.4°C
Amber
40
30.6°C
Amber
50
35.6°C
Amber
60
41.3°C
Amber
70
45.9°C
Amber
80
49.8°C
Amber
90
53.1°C
Bright red orange
100
55.5°C
Bright red orange
110
57.7°C
Bright red orange
120
59.3°C
Bright red orange
What oxidation changes does the iron undergo? Write the corresponding balanced half-reaction?
Discuss your temperature data for this reaction. How can this data be explained in light of what is happening in this experiment?
Write the balanced reaction for an oxidation-reduction reaction that happens in everyday life.
Temperature and Color Change Data for Oxidation of Iron
Time (s)
Temperature (oC)
Color observations
0
25°C
Brown
10
25.8 °C
Amber
20
26.6°C
Amber
30
28.4°C
Amber
40
30.6°C
Amber
50
35.6°C
Amber
60
41.3°C
Amber
70
45.9°C
Amber
80
49.8°C
Amber
90
53.1°C
Bright red orange
100
55.5°C
Bright red orange
110
57.7°C
Bright red orange
120
59.3°C
Bright red orange
Oxidation of Fe2+to Fe3+ 9. Measure and pour 150mL of 3% hydrogen peroxide(H2O2) into the clean 600mL beaker. 10. Use a weigh boat and scale to measure and transfer approximately 3g cream of tartar(KC4HsO) into the 600mL beaker. 11. Stir the solution with the stir rod until the cream of tartar is evenly distributed throughout the hydrogen peroxide. 12. Place the thermometer in the iron acetate solution in the flask and record the initial temperature (Time = 0) in Table 3 13. Observe and record the color of the iron acetate solution (prepared in Part 1) in Table 3" (1 g of steel wool & 4.5% Acetic Acid, C2H40) 14. Add 15 mL of the iron acetate solution from the flask to the 600 mL beaker. Record the temperature and color of the solution in Table 3 every ten seconds for two minutes; or, until you see a color change take place. You will see a marked increase in temperature as the reaction proceeds. Gently stir the solution as the reaction proceeds. Bubbles should form as carbon dioxide is released.Explanation / Answer
Q1: in the above reaction fe2+ loses one electron and convert into fe3+ its change in oxidation no is 1.
the corresponding half equation is below
The colour change also indicate the formation of Fe3+.
The
{Fe2+ = Fe3+ e}×2
H2O2 + 2H2+= 2 H2O
Overall reaction is
2fe2+ H2O2 2H+= 2 Fe3+ 2H2O
Q2: this is the indirect redox reaction in which energy is rraleased in the form of heat . an indirect redox reaction i s that in which both half take place in same container.therefore as the reaction proceed temperature rises.
Q:3 the example of redox reaction which occur in our daily life is rusting of iron in which the following reaction ocuur
2Fe. O2. 4H+= 2fe2+ 2 H2O
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