A spontaneous electrochemical cell is set up under standard conditions using Ni and Ag as electrodes - NSC Technical Sciences - Question 6 - 2021 - Paper 2
Question 6
A spontaneous electrochemical cell is set up under standard conditions using Ni and Ag as electrodes.
6.1 Choose ONE word from the statement above that indicates th... show full transcript
Worked Solution & Example Answer:A spontaneous electrochemical cell is set up under standard conditions using Ni and Ag as electrodes - NSC Technical Sciences - Question 6 - 2021 - Paper 2
Step 1
Choose ONE word from the statement above that indicates that the cell is a galvanic cell.
96%
114 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
Galvanic
Step 2
Define the following: 6.2.1 Galvanic cell
99%
104 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions.
Step 3
Define the following: 6.2.2 Electrolyte
96%
101 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
An electrolyte is a substance that dissociates into ions in solution, allowing the conduction of electricity. In electrochemical cells, it facilitates the flow of ions.
Step 4
What energy conversion will take place in the cell above?
98%
120 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The energy conversion that takes place in the cell is the conversion of chemical energy into electrical energy.
Step 5
Which ONE of the electrodes is the cathode?
97%
117 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The cathode is the Ag electrode.
Step 6
Write down the half-reaction at the cathode.
97%
121 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The half-reaction at the cathode is: Ag+ + e− → Ag.
Step 7
Calculate the emf of the cell under standard conditions.
96%
114 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
To calculate the emf of the cell, we use the formula:
Ecell=Ecathode−Eanode
Given the standard electrode potentials,
E_{cathode} = +0.80 ext{ V} ext{ (Ag$^+$ / Ag)}E_{anode} = -0.27 ext{ V} ext{ (Ni$^{2+}$ / Ni)}
Thus,
Ecell=0.80−(−0.27)=1.07extV
Step 8
Write down the cell notation for the cell above.
99%
104 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The cell notation is: Ni(s) | Ni2+(aq) || Ag+(aq) | Ag(s)
Step 9
6.8.1 Name ONE alternate energy source, besides solar energy.
96%
101 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
Wind energy.
Step 10
6.8.2 Name THREE uses of a photovoltaic cell.
98%
120 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
Powering solar panels for electricity generation.
Charging batteries in solar-powered devices.
Supplying power to grid systems as part of renewable energy infrastructure.
