Worksheetselectrochemistry
Total questions: 7
Worksheet time: 9mins
Cu2+(aq) + 2e- → Cu(s); E0 = 0.34 V
Fe3+(aq) + e- → Fe2+(aq); E0 = 0.77 V
The oxidizing and reducing agents in this galvanic cell are, respectively:
In the following half equation, which particle undergoes oxidation?
2 I- --> I2 + 2e
I-
I2
Which of the following is/are spontaneous reaction?
Please refer to Standard Reduction Potential Table.
Au3+ + Fe3+ → Fe2+ + Au
Pb + Fe3+ → Fe2+ + Pb2+
Cl2 + F- → F2 + 2Cl-
Cu2+ + 2Br- → Cu + Br2
Sn2+ + Br2 → Sn4+ + 2Br-
consider the following half equation:
Br2(l) + 2e- --> 2Br- (aq) E0 = +1.07 V
Fe2+ (aq) + 2e- --> Fe(s) E0 = -0.44 V
which of the following is a correct statement.
Fe2+ is a stronger reducing agent than Br-
Fe is a stronger reducing agent than Br2
Fe is a stronger reducing agent than Br-
Fe is stronger reducing agent than Fe2+
which of the following is a correct relative oxidising abilities of halogens
Cl2 is stronger oxidising agent compared to Br2
F2 is weaker oxidising agent compared to Cl2
aqueous Br2 can displace Cl2 from a solution of potassium chloride.
going down group 17, oxidising abilities of halogen increases
Which of the following is the correct half cell equation at anode for the spontaneous redox reaction.
Pb2+ + Fe2+ → Fe3+ + Pb
Fe3+ + e- → Fe2+
Pb2+ + 2e- → Pb
Fe2+ → Fe3+ + e-
Pb → Pb2+ + 2e-
