Question

2al + 3sn²⁺ → 2al³⁺ + 3sn which of these represents the line notation of the spontaneous cell? a. al | al³⁺(1.0 m) || sn²⁺(1.0 m) | sn b. al³⁺(1.0 m) | al || sn | sn²⁺(1.0 m) c. sn | sn²⁺(1.0 m) || al³⁺(1.0 m) | al d. sn²⁺(1.0 m) | sn || al | al³⁺(1.0 m) enter the answer choice letter.

Explanation:

To determine the line notation of a spontaneous electrochemical cell, we first identify the oxidation (anode) and reduction (cathode) half - reactions.

For the given reaction \(2\text{Al}+3\text{Sn}^{2 +}
ightarrow2\text{Al}^{3+}+3\text{Sn}\):

• Oxidation (anode): Aluminum (\(Al\)) is oxidized as its oxidation state changes from 0 in \(Al\) to + 3 in \(Al^{3+}\). The half - reaction is \(\text{Al}

ightarrow\text{Al}^{3+}+3e^-\). In line notation, the anode is written on the left, with the metal (in its elemental state) first, followed by its ion (in solution). So for the anode, we have \(\text{Al}|\text{Al}^{3 +}(1.0\ M)\).

• Reduction (cathode): Tin (\(Sn^{2+}\)) is reduced as its oxidation state changes from + 2 in \(Sn^{2+}\) to 0 in \(Sn\). The half - reaction is \(\text{Sn}^{2+}+2e^-

ightarrow\text{Sn}\). In line notation, the cathode is written on the right, with the ion (in solution) first, followed by the metal (in its elemental state). So for the cathode, we have \(\text{Sn}^{2+}(1.0\ M)|\text{Sn}\).

The double vertical line (\(||\)) in line notation represents the salt bridge, separating the anode and cathode compartments. Combining the anode and cathode notations with the salt bridge in between, we get \(\text{Al}|\text{Al}^{3+}(1.0\ M)||\text{Sn}^{2+}(1.0\ M)|\text{Sn}\), which corresponds to option A.

Answer:

A