vaazu said:1. Cr2(SO4)3 + 4K2SO4 + 3J2 +7H2O <=> K2Cr2O7 + 6KJ +7H2SO4
I used the nernst equation to calculate the potentials of
2Cr(3+)+7H2O -> Cr2O7(2-) +14H(+) +6e(-) and
I2 +2e(-) ->2J(-)
which were -1.42V and 0.51V, all ion concentrations were 0.1
Is the overall redox potential the sum of these potentials?
eli64 said:Are these J's typos, meaning I instead?
So you used the Nerst equation to calculate the half cell potentials? The Nerst equation is used to find the overall redox potential for the overall redox reaction, not half cell potential as implied here.
eli64 said:Are these J's typos, meaning I instead?
The standard half cell potentials for these half reactions are used (look up in a table) to calculate Eo, find the number of electrons transferred and use the 0.1 concentrations in the ions for the overall reaction.
Electrochemistry is a branch of chemistry that deals with the study of chemical reactions that involve the transfer of electrons between substances, also known as redox reactions. It is the study of the relationship between electricity and chemical reactions.
Redox potential, also known as oxidation-reduction potential, is a measure of the tendency of a substance to gain or lose electrons in a chemical reaction. It is a measure of the ability of a substance to act as an oxidizing agent or a reducing agent.
An electrochemical cell is a device that converts chemical energy into electrical energy or vice versa through a redox reaction. It consists of two electrodes, an anode and a cathode, which are connected by an electrolyte solution. The flow of electrons between the electrodes generates an electrical current.
Oxidation is the process of losing electrons, while reduction is the process of gaining electrons. In an oxidation-reduction reaction, one substance will be oxidized (lose electrons) while another will be reduced (gain electrons). Oxidation and reduction always occur together in a redox reaction.
The redox potential of a substance is determined by measuring the voltage produced when it is in contact with a standard hydrogen electrode. The standard hydrogen electrode has a known redox potential of 0 volts and is used as a reference point. The redox potential of a substance is then compared to the standard hydrogen electrode to determine its relative tendency to gain or lose electrons.