# data[].attributes.headline
oxidation of iron(III) ions on vanadium metal

# data[].attributes.subject
oxidation of iron(III) ions on vanadium metal

# data[].attributes.attachment_link.title
Oxidation of Iron (III) ion towards vanadium metal

# data[].attributes.body
Question:
• Drawing the set-up or apparatus
• Calculating the E° cell for a reacting using a data booklet
• Stating overall cell reaction
• Calculating the value of E using Nernst equation

Revision:
• the drawings of the set-ups of metal metal ion half cell, non-metal non-metal ion half cell and ion ion half cell
• if the half cell is ion ion, the electrode will be platinum
• if the half cell is metal metal ion, it would be the metal itself
• for making the overall equation for the reaction of the two, the number of electrons between both reactions have to be the same
• if the E value is positive, equilibrium will go to the right

# data[].attributes.body
the learnt and recall how to draw the 3 different half cells, definition of E standard, calculating the E cell, prediction of the feasibility of the reactions, faraday and nerst equation

need to learn more how to draw the 3 types of cell without referring to the textbook

teaching was great as always

# data[].attributes.body
The lecture made me feel like I should study more. The method for "(+) goes right" & "(-) goes left" was very convenient.

I think the popular questions would be "draw the cell" or "write down the components of the cells". Remembering to write the H+ seems to be important too.

# data[].attributes.body
@SHANNEN

# data[].attributes.body
Revised bout
- definition of E standard
- 3 diff half cell
- how to use data booklet to calculate volt
- how to write equation
- how to draw diagram
-nernst equation (this i need to revise cuz still cannot)

# data[].attributes.body
I learnt about some questions related to electrochemistry. Knowing how to draw the cell is very important and we need to be careful when calculating since we have to determine the right equation for the specific reagents. For example there is different reactions for Fe ions and we need to choose the right one. Other than that we also have to know how to calculate the moles of a substance using electrons. The safest electrode to answer questions is platinum but we also have to see if the electrode is another element for example Co in Co/Co2+ half cell.

# data[].attributes.body
We revised past year papers on electrochemisty, including questions on definitions, drawing and labellung diagrams, predicting the feasibility of reactions and using the Nernst equation, identifying the electrodes (note: in ion/ion cells Fe3+ uses a platinum electrode not an iron electrode) and using the Faraday constant.

# data[].attributes.body
I learnt the difference between standand cell potential and standard electrode potential. Moreover I learnt how to draw all types of half cell diagrams and also learnt that for a whole cell, a salt bridge is needed. I also learnt about the Nerst equation and that there are two types, one for standard conditions and one for other conditions which are not standard. Lastly I learnt how to calculate potential between two half-cells, the effects of LCP on the cell potential and how to calculate feasibility.

# data[].attributes.body
Revision of pyp :
- definition of standard electrode potential
- how to draw labelled diagrams to measure standard potential of cell
- how to refer to data booklet to calculate E cell
- how to predict feasibility of reactions
- how to use nernst equation and faraday
- 3 different types of ion half cell

Need to revise more on how to make equations and calculate E cell, and how to draw labelled diagrams

# data[].attributes.body
Throughout the lecture, I revised about drawing the 3 different types of half-cells. I also revised about standard electrode potential and predicting feasibility of reaction. Furthermore, I also revised about Nernst equation.

# data[].attributes.body
Expected Questions

1. Definition questions

2. Drawing and labelling the setup

3. Identifying the type of electrode used

4. Predicting the feasibility of the reaction

5. Writing the equation for the reaction

6. Predicting the change based on LCP

7. Calculating the standard cell potential

8. Calculation using the Nernst equation

# data[].attributes.body
From this lecture, I learnt

How to properly draw a labelled diagram for measuring standard electrode potential.

the conditions of a standard electrode potential.

the definition of standard electrode potential, SEP.

practice questions on the topic.

Fe 2+ is green, Fe 3+ is brown.

# data[].attributes.body
Today we practiced on solving the past year questions about this chapter. We did questions on how to draw the cell diagrams, Predicting feasibility of reactions, Nerst equations and how to calculate the electrode potential.

# data[].attributes.body
Today we revised :

When the half cell is metal/metal ions, the electrode used on one of the half cell should be the same metal in the equation.

We can use carbon or platinum or graphite as the electrode for ion/ion half cell.

Don’t forget to label the apparatus, concentrations, and ions or metals when drawing.

How to predict the feasibility of a reaction. When it is positive, it is feasible.

The more positive equation will be one top, the more negative equation’s sign will be revered and added to the other E value.

# data[].attributes.body
After going through today's revision, I have noticed a certain pattern with all the past year paper questions  —  moreover, Mr Gopi. never fails to make the lecture is very detailed but at the same time easy to understand. I think the areas that are quite popular in the past year questions are:

drawing the different types of half-cells, (metal/ metal ions, nonmetal/ non-metal ions, and ion/ ion), how to label them (don't forget the salt bridge) and identifying the electrode used

how to predict the feasibility of the reaction

definition of Standard Electrode Potential and how to calculate them

faraday constant calculations

the effect of concentration on the cell potential (use LCP)

using LCP to predict the qualitative change

questions about Nernst equation (the equation is usually given)

Overall, it was a great lecture and was not too difficult to understand.

# data[].attributes.body
after going through this revision, i felt more fond of calculating the E value, how to draw the diagrams and i understand the topic more.

the areas that i felt are more popular in the past year paper questions are usually drawing of the half cell diagrams (metal and metal ion, non metal and non metal ion, ion and ion) . Calculating the E value is also being asked quite often, calculating with the nernst equation and probably defintions of standard electrode potential.

Today’s lecture was good as usual, it was very detailed and easy to understand. Mr gopi also went through the calculation and drawing the diagrams numerous of times so we can get use to it more.

# data[].attributes.body
Questions that may come out

define standard electrode potential

draw the set up of half cells

labelling the electrode and electrolyte

calculation using Faraday's constant

calculation using nernst equation (when its not under standard conditions)

predict effect of changing concentration using LCP

# data[].attributes.body
-Reviewed the definition of standard electrode potential

-Reviewed how to draw the half cell diagrams.

-Learnt how to predict the feasibility of the reaction.

-Reviewed on the application of the nernst equation

-Learnt how to calculate equations that are not under standard conditions. (Using LCP and nernst equation)

# data[].attributes.body
Today we get to practice on how to solve the questions from this chapter. I learned how to properly draw cell diagrams, know the feasibility of reaction, how to count the E value and the nernst equation.

I think the questions that will mostly be asked are drawing and labelling the cell diagram. Counting the electrode potential or the equation that occurred in the electrodes would also be asked. Some questions may involve the nernst equation too.

The lecture was clear and detailed as usual. It clarified my doubts and helped me memorise on how to draw the diagrams.

# data[].attributes.body
Okay so today we basically just revised everything we learnt the past two-ish weeks?

I need to revise the different set-ups needed for metal/metal ions, nonmetal/nonmetal ions and gas/gas ions (as mr gopi had so kindly pointed out). As well as remembering the salt bridge.

The different questions that could come out are the definitions, calcualting electrode potential and its equations, and the set ups needed. There are also NERNST equations, w/ different conditions, also involving LCP

# data[].attributes.body
Today we reviewed:
The structure of different types of half-cells (ion-ion, metal-metal, etc)
The feasibility of a reaction and how to predict it.
Nernst Equation.
How to calculate electrode potential.

# data[].attributes.body
In this lecture, i learned how to draw the half cell diagrams especially for ions and ions, use platinum electrode and also be reminded to draw salt bridge. If equilibrium shift to the right, the E value will increase, eq shift to the leftE value will decrease

# data[].attributes.body
I revised:
1. How to properly draw cell diagrams
2. Platinum electrodes are used for ions
3. Feasibility of a reaction
4. Standard electrode potential
5. Nernst equation

A lot of drawing and freehand might be required so I need to label them properly

# data[].attributes.body
I get to know how to solve questions related to the chapter. More idea on how to answer the question and recall again the things have been told on last lecture.

# data[].attributes.body
I learned how to draw cell diagrams and how to combine half equations.

platimun rods and electrodes for ion/ion.
depending on the equation  change of concentration will affect its E value

The quetions looks to be alot of drawing and i need to draw more neatly

# data[].attributes.body
Today's lecture was mostly a review of things we've learnt in past lectures : standard electrode potential, cell potential, reaction Feasibility++

I had some questions on how to use LCP to determine changes in cell potential due to a changes in the equilibrium mixtures concerning cells that were cleared to a certain degree -, though I prolly need to read through it some more

# data[].attributes.body
revision give insight on test questions.

possible test questions
1. drawing cell diagram completely.
2. feasibility of reactions.
3. forming complete equations from half equations.
4. comparing E values to determine which gets reduced which gets oxidised. more positive mean likely to be reduced.
5. use of LCP to calculate for qualitative changes to concentration of ions or gas in the reaction.
6. nernst equation when using standard and non-standard conditions.

extra note
SEP definition: measurement of potential in equilibrium under standard conditions

# data[].attributes.body
Standard electrode potential: The measure of the potential of a half cell with reference to hydrogen half cell in standard condition which is 298K, 1atm and 1 mol/Dm^3

Three types of half cells
-Metal/metal ion
-Non-metal/non-metal ion, non metal partially submerged
-ion/ion, platinum fully submerged

Increasing the concentration of the right side of the reaction will increase the e value and increasing the concentration of the left side of the reaction will decrease the e value

Dont forget to include H+ if it is present

# data[].attributes.body
We did a bunch of past year paper questions and also reviewed on standard electrode potential.

The conditions for standard electrode potential are 1 atm of pressure in a solution of mol/dm3 with a 298K temperature.

We also reviewed the nernst equation and the feasibility of reactions.

Revision on:
- Metal and metal ion half cell
- Non-metal and non-metal ion half cell
- Ion and Ion half cell

The lecture was good as usual and the presentation is clear and concise.

# data[].attributes.body
- Practice pyp question : familiarize with the questions
* Overall equations
* Calculation using faraday [Q=IT]
* Drawing half cell diagrams
- External circuit : Electrons, Salt-Bridge : Ions
- Review LCP
- Platinum rods are expensive

Need practice :
- Calculations and overall equations

# data[].attributes.body
In this lecture, we practice some of the past year paper question. We also reviewed on standard electrode potentials, I also learned the conditions for standard electrode potential, which is 1 atm of pressure in a solution of 1 mol/dm3. We also reviewed how to predict the feasibility of the reaction. The standard electrode potential have 3 different types, metal and metal ion half cell, non metal and non metal ion half cell, and ion and ion half cell. I also learned that Nernst equation can be used under non standard condition.

# data[].attributes.body
We learned about the past year papers. We learned about electrode potentials mainly. We also learned about the drawings of the diagram, how to get the full marks. On top of that, we also learned about the Nernst equation and the calculations as well, however only for equations that are under non-standard equations. I feel like this lecture is very detailed and clear, very clear to understand. Need to remember the conditions, which is: 298 K temperature, 1 pressure atm, solution of 1 mol/dm3.

# data[].attributes.body
Conditions needed for standard electrode potential: 1atm pressure, solution 1moldm-3. Charge carriers in the solution, ions. Charge carriers in the wire, electron. Standard electrode potential is the potential of a half cell in reference to hydrogen half cell under standard condition. Nernst equation can be used for non standard condition. If there is a greater gap in E value, the prediction will be more accurate.

# data[].attributes.body
In this lesson i revised alot on electrode potentials.

When increasing or decreasing the concentration of the solution, Using LCP, we can decide wether the E value becomes more positive or more negative.
If the conentration of the ions incraese, the E value becomes more positive in most cases. Vice versa for concentration of ions decreasing.

If reaction shifts to the right, the E value will become more positive in whatever position you have the equation in.
Always remember that to never balance the E value in terms of electrons when calculating for the total E value of the two equations.

When electrolysing non-metals, The elements may be either in solid or gas form.
We sue platinum black when electrolysing nonmetal/nonmetal ions and ion/ion solutions.

WE don't use platinum rods since they are very expensive and so they fully submerge platinum electrodes when electrolysing a full aqeous solution.

be careful when choosing the equations for the half cells. When the galf equations contain a hydrogen ion, make sure to state that it is there when drawing the diagram. incldue it in the aqueous solution.

Make sure: use the correct electrode, include all the ions, Have the correct standard conditions (298K and 1mol dm^-3) and include a salt bridge.

you can use nernst equation when the reaction is happening NOT under standard conditions. eg. concentration is higher or lower than 1.

The lesson was easy to understand and i need to brush up more on the reactions and interactions of the elements related in this chapter.

# data[].attributes.body
The questions that I feel will be asked on the papers will be related to the drawing of diagrams regarding the cells and also the writing of ionic equations. They will also ask a lot about questions using the Nernst Equation, where the equation is usually given and also the effect when the amount of a certain substance is changed, answered with LCP.

# data[].attributes.body
Reviewed on :
- drawing the half cell diagrams
- faraday constant calculations ( Q=It )
- LCP ( if not in standard conditions )
- how to get marks in drawing diagrams : ex. Salt bridges, voltmeters, suitable electrolytes, etc.

Need to review more on :
Faraday constant calculations

Lecture was detailed and covered a large portion of the chapter

# data[].attributes.body
In this lecture, we practice past year paper questions. Common questions include asking for definitions and drawing diagrams. I should be reminded to draw the salt bridge (could lose 1 mark). It is also common to be asked for the overall equations and calculating using Faraday constant. I need to practice on doing calculations more. Overall, the lecture was very detailed and help revise on different types of questions.

# data[].attributes.body
In the lecture, i reviewed about past year questions. I expect questions that would ask for the definitions of SEP,etc. I also expect them to ask us to draw various types of apparatus.

Its also very common for them to ask us to write ionic equations/overall cell reaction and refer to the Data Booklet.
I need to practice on these types of questions.

The lecture was clear and detailed.

# data[].attributes.body
This lecture had clarified my doubts regarding several concepts. After going through the past year questions, I have begun to notice a pattern between the questions asked, the most common and ones I predict entailing:

1. Drawing diagrams including the two beakers, electrodes and or half cells, suitable electrolytes, a salt bridge and a voltmeter.

2. Derivation of a chemical equation from combined half equations. When in doubt, include state symbols.

3. Stating the charge carriers involved in the reaction.

4. Calculation using Faraday constant, Q = It, relation of mass, Ar and number of moles.

5. The effect caused by a difference in concentration, causing a shift in the equilibrium and the changes observed.

6. The usage of Nernst Equation to calculate EP at non-standard conditions, and how the qualitative change can be predicted using LCP.

The lecture was informative and not too difficult to follow. Recollection of past topics, IGCSE and AS Level, will aid students’ learning processes.