Home
Class 12
CHEMISTRY
The E^(0)(M^(2+)//M) value for copper is...

The `E^(0)(M^(2+)//M)` value for copper is positive `(+0.34V)`. What is possibly the reason for this?

Text Solution

AI Generated Solution

To understand why the standard electrode potential \( E^{0}(M^{2+} // M) \) for copper is positive (+0.34V), we need to analyze the energy changes involved in the process of converting copper from its solid state to its ionic form in solution. The process can be broken down into four key steps: ### Step-by-Step Solution: 1. **Sublimation Energy**: - The first step involves sublimation, which is the energy required to convert one mole of solid copper (Cu) into gaseous copper (Cu(g)). - The reaction can be represented as: \[ ...
Promotional Banner

Topper's Solved these Questions

  • THE D AND F-BLOCK ELEMENTS

    AAKASH INSTITUTE ENGLISH|Exercise Try Yourself|15 Videos

  • THE D AND F-BLOCK ELEMENTS

    AAKASH INSTITUTE ENGLISH|Exercise Assingnment(Section -A ( Objective Type Questions)(One option is correct))|50 Videos

  • Test-12

    AAKASH INSTITUTE ENGLISH|Exercise Exercise|58 Videos

  • THE P-BLOCK ELEMENTS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment Section-J)|16 Videos

Similar Questions

Explore conceptually related problems

How would you account for the following : (i) Among lanthanoids , Ln(III) compounds are predominant , However, occasionally in solutions or in solid compounds , +2 and +4 ions are also obtained . (ii) The E_(M2+//M)^(@) for copper is positive (0.34V ) . Copper is the only metal in the first series of transition elements showing this behaviour . (iii) The metallic radii of the third (5d) series of transition metals are nearly the same as those of the corresponding members of the second series .

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+) ?

E^@ for Mg to 2e^(-) + Mg^(2+) is + 2.37 V and for Cu to 2e^(-) + Cu^(+2) is -0.34V . What will be the standard potential of cell constructed with these electrodes ? Which electrode will be positive terminal to draw the current?

If E^(Theta for copper electrode is 0.34 V, how will you calculate its e.m.f. value when the solution in contact with it is 0.1M in copperions? How does e.m.f.for copper electrode changes when concentration of Cu^(2+) ions in the solution is decreased ?

A cell is prepared by dipping copper rod in 1 M copper sulphate solution and zinc rod in 1 M zinc sulphate solution. The standard reduction potential of copper and zin c are 0.34 V and - 0.76 V respectively. (i) What will be the cell reaction ? (ii) What will be the standard electromotive force of the cell ? (iii) Which electrode will be positive ?

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell

The values of some of the standard electrode potential are E^(@)(Ag^(+)//Ag)=0.80 V,E^(@)(Hg_(21+)^(2+)//Hg)=0.79 VE^(@)(Cu^(+2)//Cu)=0.34V What is the sequence of deposition of metals on the cathode ?

The potential of the cell Cu, Cu^(2+) (0.1M)"//"HCl (xM), Cl_(2), Pt is 1.07 V. If the standard potential of copper and chlorine electrodes are 0.34 V and 1.36 V, calculate the concentration of HCI.

E_(M^(3+)//(M))^(@) = -0.036V , E_(M^(2+)//M)^(@)= -0.439V . The value of standard electrode potential for the change, M^(3+)(aq) + e^(-)rightarrow M^(2+) (aq) will be :

A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The concentration of silver ions is not known.The cell potential measured is 0.422 V. Determine the concentration of silver ions in the cell. [Given E_(Ag^(+)//Ag)^(@)=0.80,E_(Cu^(2+)//Cu)^(@)=+0.34 V]