Which metal is oxidized in this case? Which metal is reduced? `Zn(S) + Cu^(2+) → Zn^(2+) + Cu(S)`

The process in which metal oxide is reduced to metal by Al is called

Represent the galvanic cell in which the reaction Is: Zn(s)+Cu^(2+) (aq) rarr Zn^(2+) (aq)+Cu(s)

The cell reaction in Daniell cell is Zn(s) + Cu^(2+) (aq) to Zn^(2+)(aq) + Cu(s) and Nernst equation for single electrode potential for general electrode reaction M^+ (aq) + n e^(-) to M(s) is E_(M^(n+)//M)=E_(M^(n+)//M)^@- (2.303 RT)/(nF) log [[M]]/[[M^(n+)]] Derive Nernst equation for Daniell cell

Which of the following oxides carnot be reduced to metal by carbon?

E^(@) for the electrochemical cell Zn(s) | Zn^(2+)1M (aq)|| Cu^(2+) 1M(aq)| Cu (s) is 1.10 V at 25^(@) C. The equilibrium constant for the cell reaction, Zn(s)+Cu^(2+) (aq.) rarr Zn^(2+) (aq.) + Cu(s) will be:

The standard E.M.F. for the cell reaction: Zn(s) + Cu^(2+) (aq) - Zn^(2+) (aq) + (Cu) is 1.10 volts at 25^(@) C. The EMF. For the cell reaction when 0.01 M Cu^(2+) and 0.1 M Zn^(2+) solutions are used at 25^(@) C is:

Which is largest in size- Cu^+ , Cu^(2+) and why?

The measured EMF at 298 K for the cell reaction, Zn(s) + Cu^(2+)(1.0 M) rarr Cu(s) + Zn^(2+)(0.1M) is 1.13 V. Calculate E^(@) for the cell reaction.

Certain elements are arranged in the order as they appear in the electrochemical series. Answer the question that follows based on this Na>Mg>Al>Zn>Cu>Ag Which of these 'metal is produced by reducing its ore with CO?