AQA A Level Chemistry
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| show | Fe2+ ——> Fe3+ + e¯
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| "Write the balanced redox half equation for the MnO4¯ being reduced to Mn2+ in acidic solution | show 🗑
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| show | " Cr2O72- + 6e¯ + 14H+ ——> 2Cr3+ + 7H2O
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| show | " "Each electrode / electrolyte combination has its own half-reaction which sets up a potential difference because different cells have a different tendency to donate or accept electrons.
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| show | "TEMPERATURE, PRESSURE OF ANY GASES, SOLUTION CONCENTRATION
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| show | "The definition of standard electrode potential E° of a half cell is the voltage of that half cell relative to a standard hydrogen electrode when all solutions have a concentration of 1 moldm-3 all gases are at 1 atmosphere and the temperature is 298K
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| " What is the Standard Electrode Potential of a standard hydrogen half cell defined as? | show 🗑
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| show | it completes the circuit by allowing the transfer of ions.
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| How does one make a salt bridge? | show 🗑
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| By convention how are all half equations written for each standard electrode potential? | show 🗑
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| If two half equations are combined how do you know what the overall reaction will be? | show 🗑
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| show | Reduced Oxidised Oxidised Reduced. ROOR
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| Write a formula to work out Ecell for a cell written in cell notation. | show 🗑
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| show | "Ecell= E° half equation for the Reduction reaction - E° half equation for the oxidation half equation.
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| " Write down the 7 rules for writing a cell in cell notation. | show 🗑
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| " Write the oxidation and reduction reactions occurring, and then write the overall reaction occurring in each cell for the Ag/Zn electrode pair. | show 🗑
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| " Calculate the standard electrode potential of the Na+/Na electrode given that when it was joined to the standard hydrogen electrode, the cell emf was –2.71 volts. | show 🗑
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| Calculate the emf of a cell with the standard AgCl/Ag electrode (Eº = +0.22 V) as the left hand electrode and the Fe2+/Fe (Eº = –0.44 V) electrode as the right hand one. | show 🗑
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| show | 0.44
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| show | 0.26
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| show | " "In theory ANY REDOX REACTION WITH A POSITIVE ECELL VALUE WILL WORK, A half equation with a more positive E° value reverse a less positive one
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| " Give two reasons why a redox reaction that is predicted to be feasible might not occur | show 🗑
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| show | They are reversed by an external current.
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| What are the pros and cons of non rechargeable batteries. | show 🗑
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| What are the pros and cons of rechargeable batteries. | show 🗑
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| show | "1 298K
2 All solutions 1moldm-3
3 All gases at 1 atmosphere pressure.
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| " What is the role of the platinum electrode in a standard hydrogen electrode | show 🗑
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| show | Zn2+/Zn equilibrium moves left releasing more electrons so making Zn2+/Zn potential more negative
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| What is the EMF of the cell created from these two half cells Zn2+(aq) + 2e– ⇌ Zn(s) E° = –0.76 V, Fe3+(aq) + e– ⇌ Fe2+(aq) E° = +0.77 V | show 🗑
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| Write the cell created by these two half cells in standard cell notation Zn2+(aq) + 2e– ⇌ Zn(s) E° = –0.76 V, Fe3+(aq) + e– ⇌ Fe2+(aq) E° = +0.77 V | show 🗑
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| show | " "iron(III) sulfate 0.5 mol dm–3 Fe2(SO4)3
iron(II) sulfate 1.0 mol dm–3 FeSO4
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| The electrode potential of the Zn2+/Zn half cell was measured against the standard hydrogen electrode (SHE). In this cell, the SHE was placed on the left, and an emf of –0.76 V was recorded. Write the standard cell notation for this cell. | show 🗑
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| "The electrode potential of the Zn2+/Zn half cell was measured against the standard hydrogen electrode (SHE). In this cell, the SHE was placed on the left, and an emf of –0.76 V was recorded. Calculate the standard electrode potential of the cell. | show 🗑
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| show | " Zn + 2H+ → Zn2+ + H2
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| show | " Fe(s) I Fe2+(aq) II Cu2+(aq) I Cu(s)
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| "Half cells for the following redox half equations were connected using a wire and salt bridge. Cu2+ + 2e– ⇌ Cu E° = +0.34 V Fe2+ + 2e– ⇌ Fe E° = –0.41 V Calculate the emf of this cell | show 🗑
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| show | Yes E cell = 1.38V
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| show | No. Ecell = -0.34V
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| show | Yes E cell = 0.29V
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