Chemical Cells & Fuel Cells Practice Questions

The student replaces the copper electrode with a second magnesium electrode.

The voltmeter now reads $0.0\ \mathrm{V}$.

Explain why.

Give two factors that affect the voltage produced by a simple cell.

The battery contains four of these cells connected in series.

Calculate the voltage produced by the battery.

Alkaline batteries are non-rechargeable.

Explain why the battery in the torch eventually stops producing a potential difference.

Use Table 1 to write the symbols of the five metals in order of reactivity.

Most reactive _______ _______ _______ _______ _______ Least reactive

The voltage measured when metal X was silver is negative.

Explain why.

The student then made a cell using a magnesium electrode and a zinc electrode in $1.0\ \mathrm{mol/dm^3}$ sodium sulfate solution.

Use Table 1 to predict the voltage produced by this cell.

Give the names of gas A and substance B in Figure 2.

Write the balanced symbol equation for the overall reaction in the hydrogen fuel cell.

The supply of gas A to the fuel cell is switched off.

Give the reason why the fuel cell stops producing a potential difference.

Write the half equation for the reaction at the negative electrode.

Write the half equation for the reaction at the positive electrode.

Explain why the reaction at the negative electrode is oxidation.

Give one reason why a hydrogen fuel cell does not need to be recharged.

Explain why the cell in the toothbrush can be recharged.

Give one environmental advantage of using rechargeable cells rather than non-rechargeable cells.

Hydrogen fuel cells offer a potential alternative to rechargeable batteries.

Evaluate the use of hydrogen fuel cell vans compared with rechargeable battery vans for the delivery company.

Use Table 2 and your own knowledge.