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Nernst Equation - to measure electric potential in non-standard conditions
E = EΘ + RT/zF ln [oxidised form]/[reduced form]
Simplified :
E = EΘ + 0,059/z log10 [oxidised form]

If [oxidised form] is > 1 mol/dm^3, E becomes less positive
If [oxidised form] is < 1 mol/dm^3, E becomes more positive

If [reduced form] is > 1 mol/dm^3, E becomes more positive
If [reduced form] is < 1 mol/dm^3, E becomes less positive

If T is not 298 K, full equation used

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Nernst equation:
• non-standard conditions
• E standard difference must be more than 0.30V
E = E standard + (RT/ZF)ln(ox/rd)

change in G = -nFecell
If E is positive, Gibbs is negative -> feasable reaction

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Predicting the feasibility of the reaction
- Strong oxi agent tendency to go right , gain electrons.
- more positive top , less positive bottom
- Positive : feasible
-Negative : Non feasible

Non standard condition
- use LCP : To find direction
-Right (more positive)
-Left (more negative)

Predicts if E standard more than 0.30V, if it is less 0.30V it cannot be predicted

Nerst equation
- Effect of conc and temp on E cells
- Oxi Form : Left
-Reduce Form : Right
- The original equation is E = Standard E + (RT/zF)•ln([ox]/[red]
- However, if the conditions are standard, the equation used is  E = Standard E + (0.059/z)•log10([ox]/[red]

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Nerst equation: E = standard E + (RT/zF) x ln(ox/red)

The simplified formula can only be used when T is 298K, otherwise use the full formula

To predict feasibility, we can use G = -nFE

When delta G is negative, the reaction is spontaneous

When value of E is positive, the reaction is feasible

Always convert kJ to J and Celsius to Kelvin

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Standard electrode potential
- Compare with standard H2 electrode
- Temp : 25 degree C

Indicate electron flow
- Indicate External circuit

Predicting the feasibility of the reaction
- SOA (Strong oxi agent) [Top] -> tendency to go right , gain electrons , stongest oxi agent
- more positive top , less positive bottom
- Positive : feasible , Negative : Non feasible

Non standard condition
- use LCP : To find direction
* Right (more positive)
* Left (more negative)

- Can only predict if E standard more than 0.30V, if it is less 0.30V it cannot be predicted

Nerst equation
- Effect of conc and temp on (Ecell)
- Oxi Form : Left , Reduce Form : Right

- Practice more ques
- learn more about nerst equation
- Remember SOA and SRA chart

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strong oxidising agent -> on the left, going to the right ( positive )
- strong reducing agent -> on the right, going to the left ( negative )
- non standard conditions -> use LCP if E standard difference is >0.30V
- nerst equation
- positive E value -> feasible
- negative E value -> non feasible

Study more on :
Nerst equations
( memorise formulas )

Teaching was good and detailed

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I learnt Nerst equation -G =nFE and can only happen under stndard condition i.e. 298k 1 atm.

I also learnt that we will be going trough a new sylabus so some material cannot be found in past papers.

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Nernst Equation:

- og formula: E = Standard E + (RT/zF)•ln([ox]/[red])
- R = gas constant
- T = temp
- z = no. Of moles
- F = Faraday constant
- applicable in non standard conditions
-" reduced form" ignored when dealing with metal/metal ions

- simplified formula : E = Standard E + (0.059/z)•lg([ox])
- simplified formula not applicable in non standard conditions

Predicting Feasibility
- negative Gibbs free energy = feasible

Formula : G = -nFE
n = number of moles
F = Faraday constant
E = standard cell potential

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NERNST Equation
- Under standard condition
E = Eø + (RT/zF) ln (Oxidized/Reduced)
R = Gas constant = 8.31

Gibbs Free Energy
- ∆Gø = - nF(Eø cell)
n = # of moles of electrons
F = Faraday = 96 500C
- If (+), reaction is feasible
- If (-), reaction is spontaneous

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Today we learnt about the NERST Equation and the equation relating the Gibbs free energy (+) and E standard.

NERST Equation:
- The original equation is E = Standard E + (RT/zF)•ln([ox]/[red]
- However, if the conditions are standard, the equation used is  E = Standard E + (0.059/z)•log10([ox]/[red]
* remember to include the concentrations of reduced ions and oxidised ions ! even if the textbook doesn't include the reduced ions concentration.

Gibbs Free Energy Equation with E standard:
- G = -nFE
- (-) bc Gibbs energy needs to be negative and E positive
- n is the amount of electrons
- F is the faraday constant: 96500
* the n here must be the number of electrons in the balanced equation. remember that the electrode potential is not multiplied or divided or whatnot, just multiplied by -1 if the equation needed to be reversed.

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Formula:

E = Standard E + RT/zF×ln( [oxidised form]/[reduce form] ).

- can be used when temp is not 298k

^ not in syllabus

E = standard E + 0.059/z × log10(oxidised form)

- temperature has to be 298k

G = -nFE

-> G has to be negative

-> F is 96500
n= number of electrons
F (Faraday) = charge on moles

Extra: to eliminate electrons, you will need to add them both but the number of electrons have to be the same

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1. Nernst equation is applicable under standard conditions

2. Use the long form of the equation when T is not 298K (the one with ln)

3. The short form of the equation can be used when T is 298K (the one with lg)

4. Predict the feasibility of an equation using G= -nFE where n is the number of electrons involved, F is Faraday, and E is the standard cell potential

5. If the value of E is positive, the reaction is feasible

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Nerst equation: E = standard E + (RT/zF) • ln(ox/red)

The simplified formula can only be used when T is 298K (the one using lg), otherwise use the full formula.

To predict feasibility, we can use G = -nFE where n = number of moles of electrons, F = faraday, and E = standard cell potential

When delta G is (-), the reaction is spontaneous

When value of E is positive, the reaction is feasible

Always convert kJ to J and Celsius to Kelvin

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I learnt about the nerst equation and there are two forms we have to remember, one form for standard temperature(298k) and the other one for other temperatures.
Moreover I also learnt about Gibbs free energy where there is a new equation G=-nFEteta. When Eteta is positive, G is negative.

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I learnt more about the Nerst equation and the 2 formulas, the simplified formula can only be used at 298k. I also learnt more about Gibbs free energy and the formula to predict feasibility is -G = -nFE, where n = number of moles, F = Faraday’s constant, which is 96500C, E = electrode potential.

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from the video i learnt:

how to apply the nernst equation, and the formula of gibs free energy and nernst equation.

simplified nernst equation can only be used at 298K, otherwise use the normal equation.

positive E value, negative gibs free energy = feasible reaction

1 faraday is 96500 Coulombs

need to always convert temperature in celcius to kelvin

always convert from Kj to Joules

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I learned about

Nerst equation: E = standard E + (RT/zF) • ln(ox/red)

Simplified formula can only be used when T is 298K

To predict feasibility: G = -nF(Ecell)

n = number of moles of electrons

F = faraday

Ecell = standard cell potential

When delta G is (-), the reaction is spontaneous

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The video taught me how to predict and calculate gibbs free energy using the equation -G = -nFE where G is Gibbs free energy, n is number of moles, F is the Faraday's constant (96500 C) and E which is the electrode potential and using the Nerst equation.

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Nernst equation, simplified version for standard temperature, but complicated version for non-standard temperature

Gibbs free energy equation for G=nFE

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I have leant the following:

1. Remember the original formula: E = Standard E + (RT/zF)•ln([ox]/[red]).

2. Simplified formula is not always applicable.

3. When ion-ion, do not remove reduced form.

4. Only use simplified formula when it is under 298K.

5. Convert temperatures in Celsius to Kelvin.

6. To predict feasibility, use the following formula: Gibbs Free Energy change = -nF(E cell).

7. When delta G (-), the reaction is spontaneous.

8. Ensure that the units are uniform (kJ to J).

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From the video, I learned more about the nernst equation
- [oxidised form]/ [reduced form] is for ion/ion
- metal don't have reduced form
- simplified formula can only be used at 298K
- 1 Faraday is 96500 colomb
- feasible reaction is not something that is fast (may require catalyst)
- negative gibbs free = feasible reaction (positive E value)
- G = - nFE (n=number of moles, F=faradays constant, E=electrode potential)

I need to memorise the equations and learn how to apply it to the questions. I also learn how to predict and calculate gibbs free energy using the E value.

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I learnt about the Nerst Equation. There are 2 formulas, the simplified one and the full one. The simplified one can only be used at 298K unlike the full formula.

I learnt about GFE( Gibbs Free Energy)

G=-nFE
where G is the Gibbs Free Energy
n=number of moles
F= Farasays constant
E= Electrode Potential

These topics is not in past papers and past textbooks so I have t memories it

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I learnt how to use the Nerst equation more clearly (difficult to write down by typing), and different variations of the equations depending on the conditions. I also learned how to calculate Gibbs Free Energy (G = -nFE) using the number of moles of electrons, Faraday's constant and standard electrode potential.

I haven't had a lot of practice doing questions on my own, so I need to practice applying the equations.

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I learnt how to predict and calculate the gibbs free energy based on the standard electrode potential, number of moles of electrons and faraday constant.

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On the video, i have learnt further about NERST Equation.
The simplified formula can only be used when T = 298K. Otherwise, use full formula.

(It is used to predict quantitatively how the value of an electrode potention would vary with the concentrations of the aqueous ions.

Then, I reviewed on feasibility
and the formula of the Gibbs free energy. (G = -nFE)

I need to:
Memorise the equations
,apply it on some questions