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Calculate the standard electrode potenti...

Calculate the standard electrode potential of `Ni^(2+)`/Ni electrode if emf of the cell `Ni_((s)) |Ni^(2+) (0.01M)| |CU^(2)| Cu _((s))(0.1M)` is `0.059 V.` `[Given : E_(Cu^(2+)//Cu)^(@) =+0.34V`

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To calculate the standard electrode potential of the `Ni^(2+)`/Ni electrode, we will follow these steps: ### Step 1: Write the cell reaction The cell reaction involves nickel and copper: \[ \text{Ni (s)} \rightarrow \text{Ni}^{2+} + 2e^- \] \[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu (s)} \] ### Step 2: Identify the anode and cathode ...
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If the standard electrode poten tial of Cu^(2+)//Cu electrode is 0.34V. What is the electrode potential of 0.01 M concentration of Cu^(2+) ?

Write the cell reaction for each of the following cells. Ni(s)|Ni^(2+)(aq)||Cu^(2+)(aq)|Cu(s).

Calculate the e.m.f. of the cell Zn//Zn^(2+) (0.1M) "||" Cu^(2+) (0.01M) "|"Cu E_(Zn^(2+)//Zn)^(Theta)= -0.76 " V and "E_(Cu^(2+)//Cu)^(Theta)=0.34V

(a) A cell is prepared by dipping a zinc rod in 1M zinc sulphate solution and a silver electrode in 1M silver nitrate solution. The standard electrode potential given : E^(@)Zn_(2+1//Zn) = -0.76V, E^(@)A_(g+//)A_(g) = +0.80V What is the effect of increase in concentration of Zn^(2+) " on the " E_(cell) ? (b) Write the products of electrolysis of aqueous solution of NaCI with platinum electrodes. (c) Calculate e.m.f. of the following cell at 298 K: "Ni(s)"//"Ni"^(2+)(0.01M)////"Cu"^(2+)(0.1M)//"Cu(s)" ["Given"E_(Ni2+//Ni)^(@) = -0.025 V E_(Cu2+//Cu)^(@) = +0.34V] Write the overall cell reaction.

Calculate the emf of the given cell: Cu/ Cu^(2+)(0.01M) ∣∣ Cu^(2+) (0.001M)∣Cu is ( E^(@)Cu^(2+) /Cu=+0.34V)

E_(Cu^(2+)//Cu)^(@) =0.43V E_(Cu^(+)//Cu)^(@)=0.55V E_(Cu^(2+)//Cu^(+))^(@) =

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

Calculate the maximum work that can be obtained from the daniell call given below, Zn(s)|Zn^(2+)(aq)||Cu^(2+)(aq)|Cu(s) . Given that E_(Zn^(2+)//Zn)^(@)=-0.76V and E_(Cu^(2+)//Cu)^(@)=+0.34V .

Write the nearest equation and calculate the e.m.f. of the following cell at 298 K Cu(s)|Cu^(2+)(0.130M)||Ag^(+)(1.00xx10^(-4)M)|Ag(s) Given :E_(Cu^(2+)//Cu)^(@)=0.34V and E_(Ag^(+)//Ag)^(@)=+0.80V

VMC MODULES ENGLISH-ELECTROCHEMISTRY-Level-0 (Long Answer Type ) (5 Marks)
  1. Calculate the standard electrode potential of Ni^(2+)/Ni electrode if ...

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