Nernst equation example

What is Nernst equation give examples?

log Kc = (nEcell)/0.0592V Thus, the relationship between the standard cell potential and the equilibrium constant is obtained. When Kc is greater than 1, the value of Ecell will be greater than 0, implying that the equilibrium favours the forward reaction.

What does the Nernst equation calculate?

The Nernst equation calculates the equilibrium potential (also referred to as the Nernst potential) for an ion based on the charge on the ion (i.e., its valence) and its concentration gradient across the membrane. Temperature also influences the Nernst potential (see Nernst equation below).

Why is Nernst equation used?

Nernst Equation – Can be used to find the cell potential at any moment in during a reaction or at conditions other than standard-state. Reaction quotient (Qc) – The mathematical product of the concentrations of the products of the reaction divided by the mathematical product of the concentrations of the reactants.

What is F in G =- nFE?

The relationship between ΔGo Δ G o and Eo is given by the following equation: ΔGo=−nFEo. Here, n is the number of moles of electrons and F is the Faraday constant (96,485Coulombsmole ).

What is Z Nernst equation?

mol1 (Joules per Kelvin per mole). T is the temperature in Kelvin (K = °C + 273.15). z is the valence of the ionic species. For example, z is +1 for Na+, +1 for K+, +2 for Ca2+, −1 for Cl, etc.

How does temperature affect Nernst equation?

The Nernst equation (Eq 11.4-13) shows that the potential is dependent on temperature; thus a small temperature change, such as 1°C, can have an effect, typically 2%, on the electrode potential [53].

What is the reaction quotient equation?

By calculating Q (products/reactants), you can compare it to the K value (products/reactants AT EQUILIBRIUM) to see if the reaction is at equilibrium or not. If Q=K, the reaction is at equilibrium.

What is the Nernst potential trying to tell us?

(The Nernst potential is the voltage which would balance out the unequal concentration across the membrane for that ion. For example, a positive voltage (+55) inside the neuron would keep the high concentration of positive Na+ ions outside the cell.

What is the difference between ∆ G and ∆ G?

∆G: Gibbs Energy ∆G is the change of Gibbs (free) energy for a system and ∆G° is the Gibbs energy change for a system under standard conditions (1 atm, 298K). Where ∆G is the difference in the energy between reactants and products.

What is E in G =- nFE?

E is related to the Gibbs energy change ΔG only by a constant: ΔG = −zFE, where n is the number of electrons transferred and F is the Faraday constant. There is a negative sign because a spontaneous reaction has a negative free energy ΔG and a positive potential E.

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