The cell notation below represents an electrochemical cell: Cu/Cu²⁺ (1 mol⋅dm⁻³) // Ag⁺ (1 mol⋅dm⁻³) / Ag 298 K/25 °C 6.1.1 What energy conversion is taking place in the above cell? 6.1.2 Write down TWO indicators from the cell notation that prove that the cell is operating under standard conditions - NSC Technical Sciences - Question 6 - 2022 - Paper 2

Firstly, the notation shows a temperature of 25 °C, which corresponds to standard conditions. Secondly, the notation specifies that the concentrations of the electrolytes are each at 1 mol⋅dm⁻³, meeting the standard conditions requirement.

At the cathode, the half-reaction can be represented as:

$ext{Ag}^+(aq) + e^- \rightarrow \text{Ag}(s)$

At the anode, the half-reaction can be expressed as:

$\text{Cu}(s) \rightarrow \text{Cu}^{2+}(aq) + 2e^-$

To determine spontaneity, we calculate the cell potential using the following equation:

$E_{cell} = E_{cathode} - E_{anode}$

Given values:

• For the cathode (Ag): $E_{Ag^+/Ag} = +0.80 ext{ V}$
• For the anode (Cu): $E_{Cu^{2+}/Cu} = +0.34 ext{ V}$

Thus: $E_{cell} = +0.80 ext{ V} - (+0.34 ext{ V}) = +0.46 ext{ V}$

Since $E_{cell}$ is positive, the reaction is SPONTANEOUS.

The reaction is classified as spontaneous because the positive cell potential ($E_{cell} = +0.46 ext{ V}$) indicates that the electrochemical process can proceed without external energy input.