A Daniel cell constructed in the laboratory. The voltage observed was `0.9V` instead of `1.10V` of the standard cell. A possible explanation is

For the cell Zn(s)|Zn^(2+)||Cu^(2+)|Cu(s) , the standard cell voltage, E^(c-)._(cell) is 1.10V . When a cell using these reagents was prepared in the lab, the measured cell voltage was 0.98V . One possible explanatino for the observed voltage is

For the cell Zn(s)|Zn^(2+)||Cu^(2+)|Cu(s) , the standard cell voltage, E^(c-)._(cell) is 1.10V . When a cell using these reagents was prepared in the lab, the measured cell voltage was 0.98V . One possible explanatino for the observed voltage is

For the cell Zn(s) | Zn^(2+) || Cu^(2+) | Cu(s) , the standard cell voltage E_("cell")^(0) is 1.10 V . When a cell using these reagents was prepared in the lab, the measured cell voltage was 0.97 V . One possible explanaiton of the observed voltage is

For the cell, Zn(s)abs(Zn^(2+))abs(Cu^(2+))Cu(s) , the standard cell voltage, E^(0)""_(cell) is 1.10 V. When a cell using these reagents was prepared in the lab, the measured cell voltage was 0.98 One possible explanation for the observed voltage is :

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.