NERNST EQUATION AND ESTANDARD RELATIONSHIP WITH GIBBS FREE ENERGY by Pooganeswari Siteram Pillai

Jonathan

2021-09-21 07:54:23 UTC

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.

Davis JC2G

2021-09-21 08:05:37 UTC

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

Lindsay JC2G

2021-09-21 08:06:39 UTC

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.

Kenneth JC2G

2021-09-21 08:10:21 UTC

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

Keira JC 2 Grace

2021-09-21 08:13:55 UTC

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.

Ella JC2G

2021-09-21 08:16:29 UTC

I have leant the following:

Remember the original formula: E = Standard E + (RT/zF)•ln([ox]/[red]).
Simplified formula is not always applicable.
When ion-ion, do not remove reduced form.
Only use simplified formula when it is under 298K.
Convert temperatures in Celsius to Kelvin.
To predict feasibility, use the following formula: Gibbs Free Energy change = -nF(E cell).
When delta G (-), the reaction is spontaneous.
Ensure that the units are uniform (kJ to J).

Nevan Kho

2021-09-21 08:18:09 UTC

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

Gibbs free energy equation for G=nFE

Raphael JC2G

2021-09-21 08:23:23 UTC

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.

Angela JC2G

2021-09-21 08:25:58 UTC

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

michelle jc2grace

2021-09-21 08:27:10 UTC

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

Kendrew JC2G

2021-09-21 08:28:09 UTC

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.

Jordan Jc2G

2021-09-21 08:31:02 UTC

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=-nFE^teta. When E^tetais positive, G is negative.

Earlene JC2G

2021-09-21 08:31:40 UTC

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

Dylan JC2G

2021-09-21 08:46:36 UTC

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

Cleantha

2021-09-21 09:41:15 UTC

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

Ashley JC2G

2021-09-21 13:47:53 UTC

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.

Jennifer JC2G

2021-09-21 13:53:54 UTC

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

Josh JC2G

2021-09-21 14:48:44 UTC

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

Justin JC2G

2021-09-21 14:59:53 UTC

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.

Jasmine JC2T

2021-09-22 01:23:26 UTC

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

Elizabeth Donna JC2T

2021-09-22 02:40:31 UTC

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

Catherine JC2T

2021-09-22 05:42:05 UTC

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

Geoffrey

2021-09-22 12:54:18 UTC

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]

Arwen_JC2 T

2021-09-22 14:41:15 UTC

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

Audrey JC2T

2021-09-23 13:11:36 UTC

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