Redox / Electrochemical cells Summary 0.0 / 5 ? ChemistryElectrode potentialsRedoxA2/A-levelAQA Created by: KaylaxlouiseCreated on: 02-05-14 21:58 What is a redox reaction? A reaction where reduction and oxidation occur simultaneously. 1 of 15 How are electrochemical cells made? By dipping two different metals in salt solutions of their own ions and connecting them by a wire and a salt bridge. 2 of 15 What is the salt bridge made from? Paper soaked in potassium nitrate (KNO3). 3 of 15 Which direction does the reaction with the more negative electrode potential go? In the direction of oxidation / backwards. 4 of 15 Which direction does the reaction with the more positive electrode potential go? In the direction of reduction / forwards. 5 of 15 What is the equation to calculate standard cell potential? E cell = E right - E left 6 of 15 What factors can influence the cell potential? Temperature, pressure and concentration. 7 of 15 What are the main features of a standard hydrogen electrode? Hydrogen gas bubbled into a solution of aqueous H+ ions. Platinum is used as the electrode. 8 of 15 Why is platinum a suitable electrode? Inert and conducts electricity. 9 of 15 What are batteries? Electrochemical cells. 10 of 15 What is the main difference between the reactions that occur in non-rechargeable batteries and rechargeable batteries? Non-rechargeable: non-reversible reactions. Rechargeable: reversible reactions. 11 of 15 What electrode is H2 fed into in a hydrogen-oxygen fuel cell? Negative electrode. 12 of 15 What electrode is the O2 fed into in a hydrogen-oxygen fuel cell? Positive electrode. 13 of 15 What type of membrane separates the electrodes and what does it do? Ion-exchange membrane. Allows H+ ions to pass through it, but not electrons. 14 of 15 What product is formed from a hydrogen-oxygen fuel cell? Water 15 of 15
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