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Electrochem practice

Quiz by Natalie Wieland

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15 questions
Show answers
  • Q1
    In the reaction MnO4 + 5Fe2+ + 8H+ --> Mn2+ + 5Fe3+ + 4H2O
    electrons are transferred from Mn2+ to Fe2+
    Fe2+ is oxidized and MnO4- is reduced
    Fe3+ is oxidized and Mn2+ is reduced
    H+ is oxidized and MnO4- is reduced
    60s
  • Q2
    The Eo for Mg --> Mg2+ + 2e- is +2.37 volts. The Eo for 2Mg2+ + 4e- --> 2 Mg is
    2.37 volts
    -4.74 volts
    4.74 volts
    -2.37 volts
    60s
  • Q3
    The function of a salt bridge (or porous barrier) in an voltaic cell is to allow ions to flow
    through the wire from reducing agent to oxidizing agent
    to keep the net charge on each side zero
    from the oxidizing side of the cell to the reducing side
    to encourage charge building up on both sides of the cell
    45s
  • Q4
    What is the value of delta Go for the reaction written below? 2MnO4- (aq) + 16 H3O+ (aq) + 5Zn (s) --> 2Mn2+ (aq) + 24H2O (l) + 5Zn2+ (aq). You are given the following standard reduction potentials for the two half-reactions. Eo (MnO4-/Mn2+) = +1.49 V. Eo (Zn2+/Zn) = -0.76 V.
    -1.92 x 10^6 J
    -2.17 x 10^6 J
    -7.04 x 10^6 J
    -1.34 x 10^6 J
    300s
  • Q5
    Given: Mg2+ + 2e- --> Mg (-2.37 V). Fe3+ + 1e- --> Fe2+ (+0.77 V). When the reaction 2Mg + Fe3+ --> 2Mg2+ + Fe2+ comes to equilibrium, the Ecell value (cell potential) becomes
    0.83 V
    0.00 V
    1.60 V
    3.14 V
    60s
  • Q6
    For the reaction Cu2+ (aq) + Zn (s) --> Zn2+ (aq) + Cu (s), Eo = +1.10 V When 1.00 mole of zinc is consumed, how many faradays are transferred?
    96,500
    96,500 x 2.00 x 6.023 x 10^23
    2.00
    96,500 x 2
    60s
  • Q7
    The galvanic cell based on the reactions Ag+ + 1e- --> Ag (Eo = +0.80 V) and Fe3+ + 1e- --> Fe2+ (Eo = +0.77 V)
    has electrons lost by Ag+ and gained by Fe2+
    has an overall cell potential difference (voltage) of +1.57 V
    has electrons flowing from Fe2+ to Ag+
    has the mass of the silver electrode decreasing as this reaction proceeds
    120s
  • Q8
    Iron can be protected from oxidation by putting it into electrical contact with a substance that is more likely to be oxidized than iron. Given the reduction potentials below, which metals could be used to protect iron? Fe2+ (aq) + 2e- --> Fe (s) (Eo = -0.44 V). Zn2+ (aq) + 2e- --> Zn (s) (Eo = -0.76 V). Cu2+ (aq) + 2e- --> Cu (s) (Eo = 0.34 V). Sn2+ (aq) + 2e- --> Sn(s) (Eo = -0.14 V). Mg2+ (aq) + 2e- --> Mg(s) (Eo = -2.37 V)
    Zn or Ag
    Sn or Cu
    Zn or Mg
    Cu or Mg
    120s
  • Q9
    Copper may be used for electroplating, with a half-reaction of Cu2+ + 2e- --> Cu. If a current of 10.0 A is applied to a Cu2+ solution for 60.0 minutes, the mass of copper plated out can be calculated as
    96,500 x (1/10.0) x (1/2.00) x (1/3600.) x 63.5
    10.00 x 3600. x (6.02 x 10^23) x (1/2.00) x 63.5
    96,500 x (1/10.0) x (1/2.00) x (1/3600.) x (1/63.5)
    10.0 x 3600. x (1/96,500) x (1/2.00) x 63.5
    300s
  • Q10
    Given the following data: Ca2+ (aq) + 2e- --> Ca(s) (Eo = -2.87 V). Zn2+ (aq) + 2e- --> Zn (s) (Eo=-0.76 V). Co2+ (aq) + 2e- --> Co(s) (Eo = -0.28 V). Sn2+ (aq) + 2e- --> Sn(s) (Eo = -0.14 V). Pb2+ (aq) + 2 e- --> Pb(s) (Eo = -0.13 V). Which of the following correctly describes the ease of oxidation of the substances listed under standard state conditions?
    Ca > Zn > Co > Sn > Pb
    Ca2+ > Zn2+ > Co2+ > Sn2+ > Pb2+
    Pb > Sn > Co > Zn > Ca
    Pb2+ > Sn 2+ > Co2+ > Zn2+ > Ca2+
    300s
  • Q11
    Ag+ + e- --> Ag (Eo = 0.80 V). Al3+ + 3e- --> Al (Eo = -1.66 V). What is the balanced equation for the spontaneous reaction?
    3Ag+ + Al --> Al3+ + 3Ag
    3Ag + Al3+ --> Al + 3Ag+
    Ag+ + Al3+ --> Al + Ag+
    Ag + Al3+ --> Al + 3Ag+
    120s
  • Q12
    Ag+ + e- --> Ag (Eo = 0.80 V). Al3+ + 3e- --> Al (Eo = -1.66 V). What is the Eocell for a voltaic cell using the two half-reactions at 25 deg C?
    -2.46 V
    +0.74 V
    +2.46 V
    -0.74 V
    120s
  • Q13
    Ag+ + e- --> Ag (Eo = 0.80 V). Al3+ + 3e- --> Al (Eo = -1.66 V). What would happen to the cell potential if NH3 were added to the silver cell and Ag(NH3)2+ forms? (so decreasing the concentration of Ag+ ions)
    increased
    cannot be determined without additional information
    reduced
    no change
    120s
  • Q14
    Which of the following statements concerning galvanic cells is/are true?
    All of the above are true
    The two half-cells are connected by a salt bridge.
    Electrons flow from the anode to the cathode.
    Reduction occurs at the cathode.
    45s
  • Q15
    Metal A is more easily oxidized than metal B. What is true of A+ and B+?
    C) If a strip of metal B is plated with metal A, the metal A plating will corrode first.
    D) Both B and C are true
    B) B+ is more easily reduced than A+
    A) A+ is more easily reduced than B+
    60s

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