Electrolysis
1. This question has 4 part(s).
1.1. A student set up an electrochemical cell using a concentrated sodium chloride solution using a current of 6 A.
State the half-equations occurring at the electrodes during the electrolysis of the concentrated aqueous solution of sodium chloride.
Cathode ..................................................................................................
Anode ....................................................................................................
1.2. Calculate the time, in minutes, to produce 2.00 dm3 of gas at the anode at standard temperature and pressure.
The Faraday constant, F = 9.65 × 104 C mol–1.
State your answer to 2 significant figures and show your working.
time = ..................... minutes
1.3. The student changed the electrolyte to a very dilute sodium chloride solution.
State what change would occur at the anode and give the half equation for the process.
1.4. In a different electrolysis experiment, copper(II) sulfate solution was electrolysed using graphite electrodes.
Table 2.1 lists electrode potentials for some electrode reactions.
Table 2.1
Electrode reaction | Eθ / V |
Cu+ + e–Cu | + 0.52 |
Cu2+ + 2e–Cu | + 0.34 |
Cu2+ + e–Cu+ | + 0.15 |
2H2O + 2e–H2 + 4OH– | – 0.83 |
O2 + 2H2O + 4e–4OH– | + 0.40 |
½O2 + 2H+ + 2e–H2O | + 1.23 |
SO42– + 4H+ + 2e–SO2 + 2H2O | + 0.17 |
S2O82– + 2e–2SO42– | + 2.01 |
Explain how the products at the anode and cathode are produced.
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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