00:01
Hello students, here in this question we have to find out the cell potential of the reaction that 6 h+ + 2cr3 +, giving 3 h2 +, 2cr3+.
00:14
We have to know that the cr3+ + is getting reduced where the hydrogen is getting oxidized.
00:25
So, the e0 cell value will be equal to e0 value of the cathode minus e0 value of the anode.
00:31
For that of the chromium it is 0 .74, for that of the oxygen it is 0.
00:36
So, the e0 value will be minus 0 .74 volt.
00:40
Okay, next we have to find out the electrode cell potential.
00:44
How we will find? the cell potential can be found out by the equation of standard cell potential value minus universal gas constant value into temperature divided by number of electrons transferred into faraday constant ln the reaction quotient.
00:58
Here it will be equal to e value will be equal to e0 cell value is minus 0 .74 volt minus the universal gas constant is 8 .314 into the temperature here we can take it as room temperature that is 298 kelvin divided by the total electrons transferred here will be 6 electrons into here the faraday constant is 96500 into ln.
01:26
Here we have to write the constant q will be equal to concentration of the oxidized form divided by the concentration of the reduced form...