Oct 08, 2021 · What is the correct Nernst equation for M2+ (aq) + 2et - M (s) at 45.C? a) E (M2+/M) + 0.31510g10 (1 / [M]+2) b) E (M2+/M) | Course Hero. IMG_20211008_110854.jpg - 5. What is the correct Nernst... This preview shows page 1 out of 1 page. End of preview.
Substituting these values in the simplified equation for Q gives a value of Q = 2. Substituting the value of Q in the Nernst equation for the Zn||Cu 2+ galvanic cell gives: 2 log 2 0.0591 E E 10 o cell cell (19) 2 0.3010 0.0591 1.10 E cell = 1.09 V (20) In general: 1. If Q > 1 then E cell < E cell 2.
Sep 28, 2019 · The Nernst equation for the given conditions can be written as follows; EM n+ /M = E o – [(2.303RT)/nF] × log 1/[Mn +] Here, E° = 0.76V; n = 2; F = 96500 C/mole [Mn +] = 2 M; R =8.314 J/K mole; T =300 K; Substituting the given values in Nernst equation we get, EZn 2+ /Zn = 0.76 – [(2.303×8.314×300)/(2×96500)] × log 1/2 = 0.76 – [0.0298 × (-0.301)]
Apr 16, 2018 · which gives. –nFE = –nFE° + RT ln Q (1-5) which can be rearranged to. (1-6) This is the very important Nernst equation which relates the cell potential to the standard potential and to the activities of the electroactive species. Notice that …
The Nernst equation is often used to calculate the cell potential of an electrochemical cell at any given temperature, pressure, and reactant concentration. The equation was introduced by a German chemist named Walther Hermann Nernst.
Limitations of Nernst Equation. The activity of an ion in a very dilute solution is close to infinity and can , therefore, be expressed in terms of the ion concentration. However, for solutions having very high concentrations, the ion concentration is not equal to the ion activity.
Here, the silver electrode acts as a cathode whereas the copper electrode serves as the anode. This is because the standard electrode potential of the silver electrode is greater than that of the copper electrode. The standard electrode potential of the cell can now be calculated, as shown below.
Concept Map. The German chemist Walther Nernst (1864-1941) was one of the giants of the early days of physical chemistry. He is known mainly for his work in thermodynamics, including that of electrochemical cells. In 1920, Nernst won the Nobel Prize in Chemistry.
The Nernst equation tells us that a half-cell potential will change by 59 millivolts per 10-fold change in the concentration of a substance involved in a one-electron oxidation or reduction; for two-electron processes, the variation will be 28 millivolts per decade concentration change.
Because chlorine is widely used as a disinfectant for drinking water, swimming pools, and sewage treatment, it is worth looking at its stability diagram. Note that the effective bactericidal agent is not Cl 2 itself, but its oxidation product hypochlorous acid HOCl which predominates at pH values below its pK a of 7.3.
For this reason, the Nernst equation cannot accurately predict half-cell potentials for solutions in which the total ionic concentration exceeds about 10 3 M.
What is the standard free energy change and equilibrium constant for the following reaction at 25 °C?
concentration cell#N#galvanic cell in which the two half-cells are the same except for the concentration of the solutes; spontaneous when the overall reaction is the dilution of the solute
The Nernst equation relates the equilibrium cell potential (also called the Nernst potential) to its concentration gradient across a membrane. An electric potential will form if there is a concentration gradient for the ion across the membrane and if selective ions channels exist so that the ion can cross the membrane.
A zinc electrode is submerged in an acidic 0.80 M Zn 2+ solution which is connected by a salt bridge to a 1.30 M Ag + solution containing a silver electrode. Determine the initial voltage of the cell at 298K.