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

What happens to the cell potential if the concentration of the oxidised species at the cathode is increased (all else constant)?

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

A student places a voltmeter across a fuel cell and observes 0.65 V under load, but the open-circuit voltage (no load) is 0.75 V. Which is the most likely cause of the 0.10 V difference?

Which half-equation correctly represents the oxidation that occurs at the anode in a hydrogen–oxygen fuel cell (acid electrolyte)?

A fuel cell produces 150 kJ of electrical energy for each 200 kJ of chemical energy in the hydrogen fuel consumed. What is the efficiency (electrical energy output / chemical energy input) expressed as a percentage?

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

Which overall reaction describes a proton exchange membrane (PEM) hydrogen fuel cell using hydrogen and oxygen?

Which statement about internal resistance in a cell is true?

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

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