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The most pupular electrochemical cell, d...


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.

A

0

B

1.1

C

1.16

D

1.04

Text Solution

Verified by Experts

The correct Answer is:
B
`E=1.1-(0.06)/(2)log(0.1)/(0.1)`
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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))

For the given cell arrangement identify incorrect statement given E^@_(Cu^(2+)//Cu) = 0.34V & E^@_(Zn^(2+)//Zn) = -0.76V

Why blue colour of CuSO_(4) solution gets discharged when zinc rod is dipped in it ? Given, E_(Cu^(+2)//Cu)^(@)=0.34 V and E_(Zn^(+2)//Zn)^(@)=-0.76V

Which is/are correct among the following? Given the half cell EMFs E_(Cu^(2+)//Cu)^(@)=0.337V, E_(Cu^(+)|Cu)^(@)=0.521V

Calculate the EMF of a Daniel cell when the concentartion of ZnSO_(4) and CuSO_(4) are 0.001M and 0.1M respectively. The standard potential of the cell is 1.1V .

Calculate the quantity of electricity dellvered by a Daniel celi initially containing 1 L each of 1M Cu^(2+) ion and 1M Zn^(2+) C which is operated until potential drops to 1V. Given E^(@) Zn^(2+)//Zn=-0.76V, E_(Cu^(2+)//Cu)^(@)=+0.34V

Can a solution of 1 M ZnSO_(4) be stored in a vessel made of copper ? Given that E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V

E^(c-)._(red) of different half cell are given as : E^(c-)._(Cu^(2+)|Cu)=0.34V,E^(c-)._(Zn^(2+)|Zn)=-0.76V . E^(c-)._(Ag^(o+)|Ag)=0.80 V, E^(c-)._(Mg^(2+)|Mg)=-2.37V. In which cell DeltaG^(c-) is most negative ?

E^(@) (SRP) of different half cell given {:(E_(Cu^(2+)//Cu)^(@) =0.34"volt",,,E_(Zn^(2+)//Zn)^(@) =- 0.76"volt"),(E_(Ag^(+)//Ag)^(@) = 0.8"volt",,,E_(Mg^(2+)//Mg)^(@) =- 2.37 "volt"):} In which cell Delta^(@) is most negative:-

A cell is constructed by dipping a zinc rod in 0.1 M zinc nitrate solution and a lead rod in 0.2 M lead nitrate solution. E_(Pb^(2+)//Pb)^(Theta) = -0.13 V and E_(Zn^(2+)//Zn)^(Theta) = -0.76V (i) Write the spontaneous cell reaction. (ii) Calculate standard emf and emf of the cell.

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