Describe an electrolytic cell with a DC power source, two electrodes and an electrolyte, explain how ions carry the current in the electrolyte and electrons in the wires, and deduce the electrode products and half-equations for the electrolysis of a molten salt.
Tę umiejętność sprawdzają 22 zadania wzorowane na arkuszach IB z lat 2022–2026.
What are the products of the electrolysis of molten lead(II) bromide? A. Product at cathode: lead; product at anode: bromine B. Product at cathode: lead; product at anode: bromide C. Product at cathode: bromine; product at anode: lead D. Product at cathode:…
Sodium ions are produced at the anode from the sodium atoms stored in the hard carbon. (i) State the half-equation for the reaction occurring at the anode while the battery discharges. (ii) The battery is rechargeable. Annotate the diagram below to show the…
Molten lead(II) bromide, PbBr2(l), is electrolysed using inert electrodes. Which products form at the electrodes? A. Anode: Br2, cathode: Pb B. Anode: O2, cathode: Pb C. Anode: Pb, cathode: Br2 D. Anode:…
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.…
Sodium metal is manufactured by the electrolysis of molten sodium chloride. (i) Outline why sodium can be produced by electrolysis rather than by reduction with carbon. (ii) State the half-equation for the formation of sodium during the electrolysis.
Molten potassium iodide is electrolysed. Write the half-equation for the reaction at each electrode: the positive electrode (anode) and the negative electrode (cathode).
What are the products of the electrolysis of molten lead(II) bromide, PbBr2(l)? A. Pb(l) + Br2(g) B. Pb2+(l) + 2 Br−(l) C. Pb2+(l) + Br2(g) D. Pb(l) + 2 Br−(l)
An electrolytic cell is made using inert electrodes and molten calcium chloride, CaCl2(l). State the half-equation for the reaction occurring at each electrode. Anode (positive electrode): Cathode (negative electrode):
Lead(II) bromide is electrolysed in the molten state at 400 °C. Lead melts at 327 °C and lead(II) bromide melts at 371 °C; bromine boils at 59 °C. Which is the correct equation for the overall reaction? A. PbBr2(l) → Pb(l) + Br2(g) B.…
Deduce the products formed at each electrode during the electrolysis of molten magnesium iodide, MgI2. Anode (positive electrode): Cathode (negative electrode):
Molten lithium bromide, LiBr(l), is electrolysed using inert graphite electrodes, as shown in the diagram. (i) Identify the product formed at the cathode. (ii) State the direction in which the electrons flow in the external circuit, referring to the…
Beryllium metal is produced by the electrolysis of beryllium chloride, BeCl2, dissolved in molten sodium chloride. (i) Write the half-equation for the process at the electrode where beryllium metal is produced. (ii) Calculate the atom economy of this…
Which statement describes a voltaic cell? A. It converts electrical energy to chemical energy using a spontaneous redox reaction B. It converts chemical energy to electrical energy using a non-spontaneous redox reaction C. It converts electrical energy to…
Which row describes an electrolytic cell? A. The anode is positive; the overall reaction is non-spontaneous B. The anode is negative; the overall reaction is spontaneous C. The anode is negative; the overall reaction is non-spontaneous D. The anode is…
A student electrolysed aqueous silver nitrate between two silver electrodes, as shown. Each electrode was washed, dried and weighed before and after the electrolysis. Suggest why the mass gained by the cathode is a less accurate measure of the amount of silver…
Aluminium has a low density, which is why it is widely used in aircraft and in specialized alloys. Aluminium is produced industrially by the electrolysis of aluminium oxide dissolved in molten cryolite, as shown in the diagram. (i) Outline why the molten…
Aluminium is a low-density metal that is used in lightweight alloys. Aluminium is produced by the electrolysis of molten aluminium oxide (in industry dissolved in molten cryolite to lower the operating temperature). A simplified cell is shown in the diagram.…
Zinc can be obtained by the electrolysis of molten zinc chloride, ZnCl2. Write the half-equation for the formation of zinc at the negative electrode.
Deduce the half-equation for the process at each electrode. Cathode (negative electrode): Anode (positive electrode):
Deduce the equation for the overall reaction in the cell, including state symbols.
Which statement is correct for the cathode in both a voltaic cell and an electrolytic cell? A. It is the positive electrode B. It is the negative electrode C. Anions move towards it D. Reduction takes place at it
Molten lead(II) bromide is electrolysed using inert graphite electrodes connected to a DC power supply. Bromine forms at one of the electrodes. Which row is correct for the electrode where bromine forms? A. Anode; positive electrode; electrons leave this…
Zapisujemy na Twoim urządzeniu to, bez czego serwis nie działa, np. zalogowanie. Plików analitycznych użyjemy tylko za Twoją zgodą. Szczegóły w polityce prywatności.