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

1. The concentration of the electrolyte is specified as 1 mol·dm⁻³, which indicates standard concentration.
2. The temperature is provided as 298 K, representing standard temperature conditions.

The balanced half-reaction at the cathode is:

The balanced half-reaction at the anode is:

To determine if the reaction is spontaneous, we can calculate the cell potential (E°cell) using:

$E°_{cell} = E°_{cathode} - E°_{anode}$

Using the provided values:

• For the cathode (Ag): E° = +0.80 V
• For the anode (Cu): E° = +0.34 V

Now substituting the values:

$E°_{cell} = 0.80 V - 0.34 V = 0.46 V$

Since E°cell is positive, the reaction is spontaneous.

The reaction is spontaneous because the standard cell potential (E°cell) is positive, indicating that the electrochemical process can occur naturally without external energy input.