Find the `EMF ` of the cell at `25^(@)C`.
`E^(c-)._(red("quinhydrone electrode ")=0.699V`
`E^(c-)._(red(" calomel electrode")=+0.268V`.

What will be the standard EMF of the cell with reaction (i) if E_(red)^0 of nickel electrode is -0.25Vand that of silver electrode is 0.8V?

The standard EMF of decinormal calomel electrode is 0.268 V . The EMF is

The standard EMF of decinormal calomel electrode is 0.268 V . The EMF is

A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of 10^(-6)M hydrogen ions. The EMF of the cell is 0.118V at 25^(@)C . Calculate the concentration of hydrogen ions at the positive electrode.

A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of 10^(-6)M hydrogen ions. The EMF of the cell is 0.118V at 25^(@)C . Calculate the concentration of hydrogen ions at the positive electrode.

The emf of the cells obtained by combining zinc and copper electrodes of the Daniell cell with calomel electrodes are 1.083 volt and -0.018 volt respectively at 25^(@)C . If the reduction potential of normal calomel electrode is + 0.28 volt, find the emf of the Daniell cell.

The e.m.f a cell is 0.265V at 25^(@)C and 0.2594V at 35^(@)C . Hence

What is the [Fe^(2+)] in a cell at 25^(@)C for which E = -0.458 V with a standard hydrogen electrode? Fe^(2+)(aq) + 2e^(-) rightarrow Fe(s) E^(@) = -0.440V

The e.m.f. of the cell obtained by combining Zn and Cu electrode of a Daniel cell with N calomel electrode in two different arrangements are 1.083V and 0.018V respectively at 25^(@)C . If the standard reduction potential of N calomel electrode is 0.28V find the emf of Daniel cell.