Chemical Cells And Fuel Cells (chemistry Only) (GCSE Chemistry)

A reversible Daniell cell is made from a zinc electrode in Zn2+ and a copper electrode in Cu2+. The standard electrode potentials are: Zn2+ + 2e- ? Zn(s) E° = -0.76 V; Cu2+ + 2e- ? Cu(s) E° = +0.34 V. What is the standard emf of the cell (Cu as cathode, Zn as anode)?

Which change will increase the voltage measured from a galvanic cell at the same temperature?

Standard hydrogen electrode (SHE) is used as the reference electrode with potential defined as 0.00 V. Which half-reaction is used for SHE?

Which advantage of a hydrogen fuel cell (using H2 and O2) compared with burning hydrogen in an engine is correct?

Which of these is a realistic safety concern when storing hydrogen for fuel cells?

Which statement about fuel cells is correct?

A simple electrochemical cell notation is: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s). Which electrode is the cathode?

A student compares an H2–O2 fuel cell with a hydrogen combustion engine. Which correct environmental advantage does the pure H2–O2 fuel cell have?

Which statement about internal resistance in a cell is true?

A student connects two identical cells in series. What happens to the total emf and the available current (assuming internal resistances are small)?

A car fuel cell stack gives lower voltage under heavy load. Which reason explains the drop?