7. Redox Reactions

Electrochemical Cells — Quiz

Test your understanding of electrochemical cells with 5 practice questions.

Practice Questions

Question 1

In a galvanic cell consisting of lead (Pb) and tin (Sn), what is the correct cell potential under standard conditions? The standard reduction potentials are $E^\circ(\text{Pb}^{2+}/\text{Pb}) = -0.13 \, V$ and $E^\circ(\text{Sn}^{2+}/\text{Sn}) = -0.14 \, V$.

Question 2

In an electrochemical cell, which of the following best explains why platinum is often used as an inert electrode?

Question 3

In a galvanic cell, what happens to the cell potential if the concentration of the reactant ions is decreased?

Question 4

In a galvanic cell made of copper (Cu) and zinc (Zn), what is the correct expression for the cell potential under non-standard conditions if $[\text{Cu}^{2+}] = 0.10 \, M$ and $[\text{Zn}^{2+}] = 1.0 \, M$? The standard reduction potentials are $E^\circ(\text{Cu}^{2+}/\text{Cu}) = +0.34 \, V$ and $E^\circ(\text{Zn}^{2+}/\text{Zn}) = -0.76 \, V$.

Question 5

In a galvanic cell involving iron (Fe) and lead (Pb), which of the following accurately represents the overall balanced cell reaction? The standard reduction potentials are $E^\circ(\text{Fe}^{2+}/\text{Fe}) = -0.44 \, V$ and $E^\circ(\text{Pb}^{2+}/\text{Pb}) = -0.13 \, V$.