(a)\(E = {E^o} - \frac{{RT}}{{nF}}\ln \frac{1}{{[{M^{n + }}]}}\); \(E = {E^o} + \frac{{RT}}{{nF}}\ln [{M^{n + }}]\) \(E = {E^o} + \frac{{2.303RT}}{{nF}}\log [{M^{n + }}]\) Substituting the value of \( R, T (298\,K) \) and \(F \) we get \(E = {E^o} + \frac{{0.0591}}{n}\log ({M^{n + }})\).
ELECTROCHEMISTRY
20076
Standard electrode potential of \(NHE\) at \(298\,K\) is .............. \(\mathrm{V}\)
1 \(0.05\)
2 \(0.1\)
3 \(0\)
4 \(0.11\)
Explanation:
(c)At \(298\,K\) standard electrode potential of \(NHE\) electrode is \( 0.00\,V\)
ELECTROCHEMISTRY
20077
When a copper wire is placed in a solution of \(AgN{O_3}\), the solution acquires blue colour. This is due to the formation of
1 \(C{u^{2 + }}\) ions
2 \(C{u^ + }\) ions
3 Soluble complex of copper with \(AgN{O_3}\)
4 \(C{u^ - }\) ion by the reduction of \(Cu\)
Explanation:
(a)Since, \(A{g^ + }\) ions are reduced to \(Ag\) and \(E_{A{g^ + }/Ag}^o > E_{C{u^{ + 2 }}/Cu}^o\) \(Cu\) is oxidized to \(C{u^{ + 2 }}\).
ELECTROCHEMISTRY
20078
Consider the reaction \(M_{(aq)}^{n + } + n{e^ - } \to {M_{(s)}}\). The standard reduction potential values of the elements \({M_1},\,{M_2}\) and \({M_3}\) are \( - 0.34V,\, - \,3.05\,V\) and \( - 1.66\,V\) respectively. The order of their reducing power will be
1 \({M_1} > {M_2} > {M_3}\)
2 \({M_3} > {M_2} > {M_1}\)
3 \({M_1} > {M_3} > {M_2}\)
4 \({M_2} > {M_3} > {M_1}\)
Explanation:
(d)The reducing power decreases as the reduction potential increase (becomes less negative).
(a)\(E = {E^o} - \frac{{RT}}{{nF}}\ln \frac{1}{{[{M^{n + }}]}}\); \(E = {E^o} + \frac{{RT}}{{nF}}\ln [{M^{n + }}]\) \(E = {E^o} + \frac{{2.303RT}}{{nF}}\log [{M^{n + }}]\) Substituting the value of \( R, T (298\,K) \) and \(F \) we get \(E = {E^o} + \frac{{0.0591}}{n}\log ({M^{n + }})\).
ELECTROCHEMISTRY
20076
Standard electrode potential of \(NHE\) at \(298\,K\) is .............. \(\mathrm{V}\)
1 \(0.05\)
2 \(0.1\)
3 \(0\)
4 \(0.11\)
Explanation:
(c)At \(298\,K\) standard electrode potential of \(NHE\) electrode is \( 0.00\,V\)
ELECTROCHEMISTRY
20077
When a copper wire is placed in a solution of \(AgN{O_3}\), the solution acquires blue colour. This is due to the formation of
1 \(C{u^{2 + }}\) ions
2 \(C{u^ + }\) ions
3 Soluble complex of copper with \(AgN{O_3}\)
4 \(C{u^ - }\) ion by the reduction of \(Cu\)
Explanation:
(a)Since, \(A{g^ + }\) ions are reduced to \(Ag\) and \(E_{A{g^ + }/Ag}^o > E_{C{u^{ + 2 }}/Cu}^o\) \(Cu\) is oxidized to \(C{u^{ + 2 }}\).
ELECTROCHEMISTRY
20078
Consider the reaction \(M_{(aq)}^{n + } + n{e^ - } \to {M_{(s)}}\). The standard reduction potential values of the elements \({M_1},\,{M_2}\) and \({M_3}\) are \( - 0.34V,\, - \,3.05\,V\) and \( - 1.66\,V\) respectively. The order of their reducing power will be
1 \({M_1} > {M_2} > {M_3}\)
2 \({M_3} > {M_2} > {M_1}\)
3 \({M_1} > {M_3} > {M_2}\)
4 \({M_2} > {M_3} > {M_1}\)
Explanation:
(d)The reducing power decreases as the reduction potential increase (becomes less negative).
(a)\(E = {E^o} - \frac{{RT}}{{nF}}\ln \frac{1}{{[{M^{n + }}]}}\); \(E = {E^o} + \frac{{RT}}{{nF}}\ln [{M^{n + }}]\) \(E = {E^o} + \frac{{2.303RT}}{{nF}}\log [{M^{n + }}]\) Substituting the value of \( R, T (298\,K) \) and \(F \) we get \(E = {E^o} + \frac{{0.0591}}{n}\log ({M^{n + }})\).
ELECTROCHEMISTRY
20076
Standard electrode potential of \(NHE\) at \(298\,K\) is .............. \(\mathrm{V}\)
1 \(0.05\)
2 \(0.1\)
3 \(0\)
4 \(0.11\)
Explanation:
(c)At \(298\,K\) standard electrode potential of \(NHE\) electrode is \( 0.00\,V\)
ELECTROCHEMISTRY
20077
When a copper wire is placed in a solution of \(AgN{O_3}\), the solution acquires blue colour. This is due to the formation of
1 \(C{u^{2 + }}\) ions
2 \(C{u^ + }\) ions
3 Soluble complex of copper with \(AgN{O_3}\)
4 \(C{u^ - }\) ion by the reduction of \(Cu\)
Explanation:
(a)Since, \(A{g^ + }\) ions are reduced to \(Ag\) and \(E_{A{g^ + }/Ag}^o > E_{C{u^{ + 2 }}/Cu}^o\) \(Cu\) is oxidized to \(C{u^{ + 2 }}\).
ELECTROCHEMISTRY
20078
Consider the reaction \(M_{(aq)}^{n + } + n{e^ - } \to {M_{(s)}}\). The standard reduction potential values of the elements \({M_1},\,{M_2}\) and \({M_3}\) are \( - 0.34V,\, - \,3.05\,V\) and \( - 1.66\,V\) respectively. The order of their reducing power will be
1 \({M_1} > {M_2} > {M_3}\)
2 \({M_3} > {M_2} > {M_1}\)
3 \({M_1} > {M_3} > {M_2}\)
4 \({M_2} > {M_3} > {M_1}\)
Explanation:
(d)The reducing power decreases as the reduction potential increase (becomes less negative).
(a)\(E = {E^o} - \frac{{RT}}{{nF}}\ln \frac{1}{{[{M^{n + }}]}}\); \(E = {E^o} + \frac{{RT}}{{nF}}\ln [{M^{n + }}]\) \(E = {E^o} + \frac{{2.303RT}}{{nF}}\log [{M^{n + }}]\) Substituting the value of \( R, T (298\,K) \) and \(F \) we get \(E = {E^o} + \frac{{0.0591}}{n}\log ({M^{n + }})\).
ELECTROCHEMISTRY
20076
Standard electrode potential of \(NHE\) at \(298\,K\) is .............. \(\mathrm{V}\)
1 \(0.05\)
2 \(0.1\)
3 \(0\)
4 \(0.11\)
Explanation:
(c)At \(298\,K\) standard electrode potential of \(NHE\) electrode is \( 0.00\,V\)
ELECTROCHEMISTRY
20077
When a copper wire is placed in a solution of \(AgN{O_3}\), the solution acquires blue colour. This is due to the formation of
1 \(C{u^{2 + }}\) ions
2 \(C{u^ + }\) ions
3 Soluble complex of copper with \(AgN{O_3}\)
4 \(C{u^ - }\) ion by the reduction of \(Cu\)
Explanation:
(a)Since, \(A{g^ + }\) ions are reduced to \(Ag\) and \(E_{A{g^ + }/Ag}^o > E_{C{u^{ + 2 }}/Cu}^o\) \(Cu\) is oxidized to \(C{u^{ + 2 }}\).
ELECTROCHEMISTRY
20078
Consider the reaction \(M_{(aq)}^{n + } + n{e^ - } \to {M_{(s)}}\). The standard reduction potential values of the elements \({M_1},\,{M_2}\) and \({M_3}\) are \( - 0.34V,\, - \,3.05\,V\) and \( - 1.66\,V\) respectively. The order of their reducing power will be
1 \({M_1} > {M_2} > {M_3}\)
2 \({M_3} > {M_2} > {M_1}\)
3 \({M_1} > {M_3} > {M_2}\)
4 \({M_2} > {M_3} > {M_1}\)
Explanation:
(d)The reducing power decreases as the reduction potential increase (becomes less negative).