Explain that rechargeable cells run spontaneous redox reactions on discharge that are reversed by an applied current on charging, and deduce the charging reactions by reversing given discharge electrode reactions, and vice versa.
Tę umiejętność sprawdza 11 zadań wzorowanych na arkuszach IB z lat 2023–2026.
Iron and nickel can be used to design a voltaic cell. Fe(s) + Ni2+(aq) → Fe2+(aq) + Ni(s) (i) Annotate the diagram with the appropriate electrodes, electrolyte solutions and the direction of electron flow. (ii) The redox reactions in some voltaic…
During discharge, sodium atoms stored in the hard carbon are converted into sodium ions. (i) State the half-equation for the process taking place at the anode while the battery discharges. (ii) With reference to section 19 of the data booklet, comment on the…
The diagram below shows the battery connected to a charger. Annotate the diagram to show the direction in which electrons flow through the external wires while the battery is being recharged.
Suggest why banks of sodium-ion batteries are often installed alongside wind turbines.
(i) In the nickel–metal hydride (NiMH) rechargeable battery the negative electrode is a metal alloy, M, that absorbs hydrogen. The two electrode reactions during discharge are shown below.…
Which statement correctly describes a type of electrochemical cell? A. A secondary cell operates as a voltaic cell when discharging and as an electrolytic cell when it is recharged B. A primary (voltaic) cell converts electrical energy into chemical energy C.…
Below is a sodium-ion cell as it discharges, supplying a current to an external circuit. The anode is sodium held in a lattice of hard carbon and the cathode is iron(III) phosphate, FePO4, which is converted to NaFePO4 as the cell discharges.…
The overall reaction during the discharge of a lead–acid battery is: Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(l) Which statement is correct? A. The oxidation state of lead in Pb(s) changes from +2 to 0. B. The oxidation state of sulfur…
A lithium-ion cell in a mobile phone can be recharged, but a zinc–carbon cell in a torch cannot. Outline why.
Describe, in detail, how a hydrogen–oxygen fuel cell and a secondary cell can each be used again and again without being replaced. Fuel cell: Secondary cell:
A hydrogen fuel cell and a rechargeable lithium-ion cell can both be used to supply electricity again and again. Describe, for each type of cell, what must be done so that it can be used again after the cell can no longer supply electricity.
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