Writing Redox Equations from Half-Equations (A Level) Quiz

Derived lesson quiz from the Electrochemistry bank focused on half-equation logic, balancing strategy, and redox equation assembly.

GCE A-Level H2 Chemistry 9476-2027

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When balancing electrons by multiplying half-equations, what should you do to the $E^\ominus$ values?

Multiply $E^\ominus$ by the same factor
Divide $E^\ominus$ by the same factor
Do not change $E^\ominus$ values
Add the $E^\ominus$ values directly

Given $E^\ominus(\ce{Cu^{2+}/Cu})=+0.34\ \text{V}$ and $E^\ominus(\ce{Zn^{2+}/Zn})=-0.76\ \text{V}$, which species is the oxidising agent in the spontaneous cell?

$\ce{Zn(s)}$
$\ce{Zn^{2+}}$
$\ce{Cu(s)}$
$\ce{Cu^{2+}}$

Using $E^\ominus(\ce{Cu^{2+}/Cu})=+0.34\ \text{V}$ and $E^\ominus(\ce{Zn^{2+}/Zn})=-0.76\ \text{V}$, what is $E^\ominus_{cell}$ for the $\ce{Zn/Cu}$ cell?

0.42 V
1.10 V
−1.10 V
−0.42 V

Molten $\ce{NaCl}$ is electrolysed using inert electrodes. What are the electrode products?

Cathode: $\ce{H2}$, Anode: $\ce{O2}$
Cathode: $\ce{Na}$, Anode: $\ce{Cl2}$
Cathode: $\ce{Cl2}$, Anode: $\ce{Na}$
Cathode: $\ce{NaOH}$, Anode: $\ce{HCl}$

In electrolysis of concentrated aqueous $\ce{NaCl}$ with inert electrodes, the main gas at the anode is usually:

$\ce{H2}$
$\ce{O2}$
$\ce{Cl2}$
$\ce{CO2}$

In electrolysis of aqueous $\ce{CuSO4}$ using inert electrodes, what happens at the cathode?

$\ce{2H2O + 2e- -> H2 + 2OH-}$
$\ce{Cu^{2+} + 2e- -> Cu}$
$\ce{2SO4^{2-} -> S2O8^{2-} + 2e-}$
$\ce{2Cl- -> Cl2 + 2e-}$

Which statement is always true (galvanic cells and electrolysis)?

Anode is always positive
Cathode is always negative
Oxidation occurs at the anode and reduction occurs at the cathode
Electrons flow from cathode to anode in the external circuit

What is the overall reaction in a hydrogen–oxygen fuel cell?

$\ce{2H2 + O2 -> 2H2O}$
$\ce{2H2O -> 2H2 + O2}$
$\ce{H2 + O2 -> H2O2}$
$\ce{H2 + O2 -> H2O}$

Writing Redox Equations from Half-Equations (A Level) Quiz

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