On the basis of the electron transfer, explain which ion is getting oxidised and which getting reduced in the following reactions :
`2Cu^(2+)+4l^(-)to2Cu l+I_(2)`

On the basis of the electron transfer, explain which ion is getting oxidised and which getting reduced in the following reactions : 2Fe^(3+)+S^(2-)to2Fe^(2+)+S

Redox is a reaction in which both oxidation and reduction will take place simultaneously . It is obvious that if one substance gives electron there must be another substance to accept these electrons . In some reactions, same substance is reduced as well as oxidised, these reactions are termed as disproportionation reactions. For calculating equivalent mass in redox reaction change in oxidtaion number is realted to n-factor which is reciprocal of molar ratio. The equivalent weight of Cu_(2)S in the following reaction is Cu_(2)S + O_(2) to Cu^(+2) + SO_(3)

Identify the substances that are oxidised and the substances that are reduced in the following reactions. (i) 4Na(s)+O_(2)(g)rarr2NaO(s) (ii) CuO(g) +H_(2)(g) rarr Cu(s) +H_(2)O(l)

Which of the following is electronic configuration of Cu^(2+) (Z = 29) ?

Divide the following redox reactions into oxidation and reduction half reactions. Zn + Cu^(2+) to Zn&(2+) + Cu

Write Nernst equation for the following cell reaction : Zn"|"Zn^(2+)(aq)"||"Cu^(2+)(aq)"|"Cu(s)

State whether the following conversions are oxidation or reduction reactions. Cu^(2+) + 2e^(-) to Cu

the correct electronic configuration of Cu^(2+) ion is

Depict the galvanic cell in which the cell reaction is Cu+2Ag^(+)rarr2Ag+Cu^(2+)