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Find the EMF of cell (in volts) formed b...

Find the EMF of cell (in volts) formed by connected two half cells:
`Pt(s) | MnO_(4)^(-)`(0.1 M), `MnCl_(2)`(0.2M) HCl (1 M)
Pt(s) | `Cr_(2)O_(7)^(2-)(0.1M)` `CrCl_(3)`(0.2M) HCl (0.7 M)`
[Given `E_(MnO_(4)^(-)|Mn^(2+))^(@)` =1.51 V,
`E_(Cr_(2)O_(7)^(2-)| Cr^(3+) = 1.33 V]`
Give your answer by multiplying with 10.

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Calculate the potential of the following cell : Pt(s)|{:(Ce^(3+),(2M)) ,(Ce^(4+),(1M)):}||{:(Cr^(3+)(2M),) ,(Cr_(2)O_(7)^(2-)(1M),H^(o+)(1M)):}|Pt(s) Given :E^(c-)._(Ce^(3+)|Ce^(4+))=-1.7,E^(c-)._(Cr_(2)O_(7)^(2-)|Cr^(3+))=1.3V ( Take 0.059~~0.06)

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Using the data given below: E_(Cr_(2)O_(7)^(2-)|Cr^(3+))^(@)=1.33V E_(Cl_(2)|Cl^(-))^(@)=1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=1.51V E_(Cr^(3+)|Cr)=-0.74V Find the most stable ion in its reduced forms

Using the data given below: E_(Cr_(2)O_(7)^(2-)|Cr^(3+))^(@)=1.33V E_(Cl_(2)|Cl^(-))^(@)=1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=1.51V E_(Cr^(3+)|Cr)=-0.74V Find the most stable oxidised species.

Using the data given below: E_(Cr_(2)O_(7)^(2-)|Cr^(3+))^(@)=1.33V E_(Cl_(2)|Cl^(-))^(@)=1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=1.51V E_(Cr^(3+)|Cr)=-0.74V Mark the strongest reducing agent.

Using the data given below: E_(Cr_(2)O_(7)^(2-)|Cr^(3+))^(@)=1.33V E_(Cl_(2)|Cl^(-))^(@)=1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=1.51V E_(Cr^(3+)|Cr)=-0.74V Mark the strongest oxidising agent.

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