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

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

Which of the following is a correct disadvantage of fuel cells compared with conventional internal combustion engines?

Which process will reduce the voltage (terminal potential) available from a chemical cell in practical use?

In a fuel cell using an alkaline electrolyte, which ions move through the electrolyte from the cathode to the anode?

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

Which calculation correctly gives the electrical energy (in joules) delivered by a cell of emf 1.2 V supplying 2.0 A for 30 s?

Which statement about fuel cells is correct?

Which statement about internal resistance in a cell is true?

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)?

In a hydrogen fuel cell using a polymer electrolyte membrane, what is the role of the membrane?