In the following redox reaction `Cu(OH)_(2) (s) + N_(2) H_(4)(aq) rarr Cu(s) + N_(2)(g)` number of mole of `Cu(OH)_(2)` reduced by one mol of `N_(2) H_(4)` is -

Justify the following reactions are redox reaction : CuO(s) + H_2 (g) rarr Cu (s) + H_2O(g)

Justify the following reaction is a redox reaction. CuO_((s)) + H_(2(g)) to Cu_((s)) + H_(2)O_((g))

Justify that the reaction is a redox reaction. " "2Cu_(2)O(s)+Cu_(2)S(s) rarr 6Cu(s)+SO_(2)(g)

Justify that the reaction is a redox reaction. " "2Cu_(2)O(s)+Cu_(2)S(s) rarr 6Cu(s)+SO_(2)(g)

Suggest a scheme of classification of the following redox reactions (a) N_(2) (g) + O_(2) (g) rarr 2 NO (g) (b) 2 Pb (NO_(3))_(2) (s) rarr 2 PbO (s) + 4 NO_(2) (g) + O_(2) (g) (c) NaH(s) + H_(2) O (l) rarr NaOH (aq) + H_(2) (g) (d) 2NO_(2) (g) + 2OH^(-) (aq) rarr NO_(2)^(-) (aq) + NO_(3)^(-) (aq) + H_(2) O (l)

The reaction Co(s) + Cu^(2+)(aq) rarr Co^(2+)(aq) + Cu(s) is-

Write balanced net ionic equations for the following reactions in basic solution: (a) H_(2)O_(2)(aq)+ClO_(4)^(Ө)(aq) rarr ClO_(2)^(Ө)(aq)+O_(2)(g) (b) ( c) Cu(OH)_(2)(s) + N_(2)H_(4)(aq) rarr Cu(s)+N_(2)(g) (d) MnO_(4)^(Ө) + IO_(3)^(Ө)(aq)rarr MnO_(2)(s) + IO_(4)^(Ө)(aq)

Identify oxidant in reaction given below : CuO(s)+ H_(2)(g) rarr Cu(s)+H_(2)O(g)

In the following unbalanced redox reaction, Cu_(3)P+Cr_(2)O_(7)^(2-) rarr Cu^(2+)+H_(3)PO_(4)+Cr^(3+) Equivalent weight of H_(3)PO_(4) is