Standard Electrode Potentials E⦵, Standard Cell Potentials E⦵cell & the Nernst Equation
1. This question has 4 part(s).
1.1. The standard electrode potentials for seven different redox systems are shown in Table 3.1.
Table 3.1
redox system | equation | Eθ / V |
1 | 2H+ (aq) + 2e– H2 (g) | 0.00 |
2 | Fe3+ (aq) + e– Fe2+ (aq) | +0.77 |
3 | Cu2+ (aq) + 2e– Cu (s) | +0.34 |
4 | Cl2 (aq) + 2e– 2Cl– (aq) | +1.36 |
5 | O2 (g) + 4H+ (aq) + 4e– 2H2O (l) | +1.23 |
6 | Al3+ (aq) + 3e– Al (s) | -1.66 |
7 | I2 (aq) + 2e– 2I– (aq) | +0.54 |
An electrochemical cell can be made based on redox systems 2 and 3.
i) Write the overall cell reaction.
[1]
ii) Calculate the voltage of this cell.
[1]
1.2. i) Using redox systems 5, 6 and 7 only in Table 3.1, write the overall equations for three reactions that might be feasible.
[3]
ii) Give two reasons why these reactions might not take place, even if they are feasible.
[2]
1.3. Select from Table 3.1,
i) an oxidising agent that oxidises Fe2+ (aq) to Fe3+ (aq),
[1]
ii) a species that reduces Fe3+ (aq) to Fe2+ but does not reduce Cu2+ (aq) to Cu (s).
[1]
1.4. Calculate the electrode potential at 298 K of redox system 3 if the concentration of Cu2+ (aq) ions was 0.0002 mol dm-3.
Ai এর মাধ্যমে
১০ লক্ষ+ প্রশ্ন ডাটাবেজ
প্র্যাকটিস এর মাধ্যমে নিজেকে তৈরি করে ফেলো
উত্তর দিবে তোমার বই থেকে ও তোমার মত করে।
সারা দেশের শিক্ষার্থীদের মধ্যে নিজের অবস্থান যাচাই
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