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Four metals Pb, x, y and z, were connected in pairs and the voltage was recorded The results obtained are set out in the table below, | Negative terminal | Positive terminal | Voltage (V) | |------------------|------------------|-------------| | Pb | x | 0.35 | | y | Pb | 1.10 | | z | Pb | 2.60 | What is the order of increasing ease of oxidation of the metals? - HSC - SSCE Chemistry - Question 14 - 2004 - Paper 1
Question 14
Four metals Pb, x, y and z, were connected in pairs and the voltage was recorded The results obtained are set out in the table below, | Negative terminal | Positiv... show full transcript
Worked Solution & Example Answer:Four metals Pb, x, y and z, were connected in pairs and the voltage was recorded The results obtained are set out in the table below, | Negative terminal | Positive terminal | Voltage (V) | |------------------|------------------|-------------| | Pb | x | 0.35 | | y | Pb | 1.10 | | z | Pb | 2.60 | What is the order of increasing ease of oxidation of the metals? - HSC - SSCE Chemistry - Question 14 - 2004 - Paper 1
Step 1
Identify the oxidation potentials
Answer
From the given voltages, we can determine the relative ease of oxidation for each metal:
- When Pb is connected to x, the voltage is 0.35 V, indicating that Pb is losing electrons (oxidation).
- In the pair of y and Pb, the voltage is 1.10 V, thus indicating that y is losing electrons more easily compared to Pb.
- In the pair of z and Pb, the voltage is 2.60 V, indicating z is losing electrons even more easily than both Pb and y.
Step 2
Rank the metals by oxidation
Answer
Thus, we can rank the metals based on their ease of oxidation:
- z has the highest ease of oxidation (most negative), followed by y, and finally Pb. x's relative position can be inferred based on the 0.35 V with Pb but is not identified as the strongest oxidizing agent overall.
Step 3