The most pupular electrochemical cell, daniel cell was originally developed by the English chemist john F daniel the general assembly of the cell is as given below An undergraduate student made a Daniel cell using `100cm^(3)` of `0.100MCuSO_(4)` ad `0.100M` `ZnSO_(4)` solution respectively. The two compartments are connected by suitable salt bridge.
[given `E_((Cu^(2+)//Cu))^(@)=0.34V,E_((Zn^(2+)//Zn))=-0.76V,(2.30RT)/(F)=0.06,log2=0.3]`
Q. Calculate the emf (in volt) of the above cell.

The most pupular electrochemical cell, daniel cell was originally developed by the English chemist john F daniel the general assembly of the cell is as given below An undergraduate student made a Daniel cell using 100cm^(3) of 0.100MCuSO_(4) ad 0.100M ZnSO_(4) solution respectively. The two compartments are connected by suitable salt bridge. [given E_((Cu^(2+)//Cu))^(@)=0.34V,E_((Zn^(2+)//Zn))=-0.76V,(2.30RT)/(F)=0.06,log2=0.3] Q. A labmate of the student asked her for some solid CuCl_(2) . while she was lifting the bottle from a shelf, the lid of the bottle slipped and some amount of CuCl_(2) fell in the CuSO_(4) compartment at constant volume. She measured the emf of the cell again and found that it has increase by 9 mV. She used this data to calculate the amount of CuCl_(2) that had spilled in the compartment. Calculate the mass of CuCl_(2) that had spilled into the daniel cell? (molar mass of CuCl_(2)=135(g)/(mol))

The most pupular electrochemical cell, daniel cell was originally developed by the English chemist john F daniel the general assembly of the cell is as given below An undergraduate student made a Daniel cell using 100cm^(3) of 0.100MCuSO_(4) ad 0.100M ZnSO_(4) solution respectively. The two compartments are connected by suitable salt bridge. [given E_((Cu^(2+)//Cu))^(@)=0.34V,E_((Zn^(2+)//Zn))=-0.76V,(2.30RT)/(F)=0.06,log2=0.3] Q. A labmate of the student asked her for some solid CuCl_(2) . while she was lifting the bottle from a shelf, the lid of the bottle slipped and some amount of CuCl_(2) fell in the CuSO_(4) compartment at constant volume. She measured the emf of the cell again and found that it has increase by 9 mV. She used this data to calculate the amount of CuCl_(2) that had spilled in the compartment. Calculate the mass of CuCl_(2) that had spilled into the daniel cell? (molar mass of CuCl_(2)=135(g)/(mol))

The emf (in V) of a Daniell cell containing 0.1 M ZnSO_(4) and 0.01 M CuSO_(4) solutions at their respective electrodes is (E_((Cu^(2+))/(Cu))^@ = +0.34 V, E_((Zn^(2+))/(Zn))^@ = -0.76 V)

The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

Determine the EMF of a decimolar Daniell cell at 25^(@)C . Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V .