You need to keep the homework template in place on homeworks please. Also welcome to PF.
## \\ ## Additional note: The lowest line on your notes should read: ## 2MnO_4^-+8H^++6e^- \rightarrow 2MnO_2+4H_2O=(MnO_4^-+4H^++3e^- \rightarrow MnO_2+2H_2O )## x ##2 ##, in order to arrive at the ## z=6 ## in the Nernst equation. (You incorrectly have ## 3e^- ## in the same equation that has ## 8H^+ ##). Also, one more minor correction: you wrote ## [Cu^{++}]^2 ## instead of ## [Cu^{++}]^3 ##, but you correctly wrote ## (.01)^3 ## when you computed it in the next line. ## \\ ## One additional suggestion would be to call the EMF's ## \mathcal{E}_{cell}^o ## and ## \mathcal{E}_{cell} ## to distinguish the two. Initially, it was very difficult to follow what you were trying to compute.E cell refers to the standard cell potential, also known as the standard electromotive force (EMF), of a chemical reaction. It is a measure of the energy difference between the reactants and products in a redox reaction.
E cell can be calculated using the Nernst equation, which takes into account the standard electrode potentials of the half-reactions involved in the redox reaction, as well as the concentrations of the reactants and products.
Calculating E cell allows us to determine the direction and strength of a redox reaction. It also provides insight into the feasibility and spontaneity of a reaction, as well as the amount of electrical energy that can be generated.
E cell is typically measured in volts (V) or millivolts (mV).
The accuracy of E cell calculations can be affected by temperature, pH, and the presence of impurities or other interfering substances in the reaction solution. Additionally, any errors in measuring concentrations or standard electrode potentials can also impact the accuracy of the calculated E cell value.
