20083
When a rod of metal \(A\) is dipped in an aqueous solution of metal \(B\) (concentration of \({B^{2 + }}\) ion being \(1\,M\) ) at \({25\,^o}C\), the standard electrode potentials are \({A^{2 + }}/A\) \( = -0.76 \) volts, \({B^{2 + }}\) \(/B = + 0.34\) volts
1 \(A\) will gradually dissolve
2 \(B\) will deposit on \(A\)
3 No reaction will occur
4 Water will decompose into \({H_2}\) and \({O_2}\)
Explanation:
(b)Since \(E_{{A^{2 + }}/A}^o < E_{{B^{2 + }}/B}^o\). A has greater tendency to be oxidized. \(A + {B^{2 + }} \to {A^{2 + }} + B\).
ELECTROCHEMISTRY
20084
The reaction \(Z{n^{2 + }} + 2{e^ - } \to Zn\) has a standard potential of \( - 0.76\,V\). This means
1 \(Zn\) can't replace hydrogen from acids
2 \(Zn\) is a reducing agent
3 \(Zn\) is a oxidising agent
4 \(Z{n^{2 + }}\)is a reducing agent
Explanation:
(b)Since \(E_{Z{n^{ + + }}/Zn}^o\) is negative, so \(Zn\) has greater tendency to be oxidized than hydrogen. Hence it can act as reducing agent.
ELECTROCHEMISTRY
20085
\(2{H^ + }\,(aq) + 2{e^ - }\, \to \,{H_2}\,(g).\)The standard electrode potential for the above reaction is (in volts)
1 \(0\)
2 \(+1\)
3 \(-1\)
4 None of these
Explanation:
(a)Standard electrode potential of Hydrogen is zero.
ELECTROCHEMISTRY
20086
\(K,\,\,Ca\) and \(Li\) metals may be arranged in the decreasing order of their standard electrode potentials as
1 \(K,\,\,Ca,\,\,Li\)
2 \(Ca,\,\,K,\,\,Li\)
3 \(Li,\,\,Ca,\,\,K\)
4 \(Ca,\,\,Li,\,\,K\)
Explanation:
(b)According to electrochemical series.
ELECTROCHEMISTRY
20087
The correct order of chemical reactivity with water according to electrochemical series
1 \(K > Mg > Zn > Cu\)
2 \(Mg > Zn > Cu > K\)
3 \(K > Zn > Mg > Cu\)
4 \(Cu > Zn > Mg > K\)
Explanation:
(a)The standard reduction potential of \({K^ + }\), \(M{g^{2 + }},\,\,\,Z{n^{ + 2}}\,\,C{u^{2 + }}\) increase in this order.
20083
When a rod of metal \(A\) is dipped in an aqueous solution of metal \(B\) (concentration of \({B^{2 + }}\) ion being \(1\,M\) ) at \({25\,^o}C\), the standard electrode potentials are \({A^{2 + }}/A\) \( = -0.76 \) volts, \({B^{2 + }}\) \(/B = + 0.34\) volts
1 \(A\) will gradually dissolve
2 \(B\) will deposit on \(A\)
3 No reaction will occur
4 Water will decompose into \({H_2}\) and \({O_2}\)
Explanation:
(b)Since \(E_{{A^{2 + }}/A}^o < E_{{B^{2 + }}/B}^o\). A has greater tendency to be oxidized. \(A + {B^{2 + }} \to {A^{2 + }} + B\).
ELECTROCHEMISTRY
20084
The reaction \(Z{n^{2 + }} + 2{e^ - } \to Zn\) has a standard potential of \( - 0.76\,V\). This means
1 \(Zn\) can't replace hydrogen from acids
2 \(Zn\) is a reducing agent
3 \(Zn\) is a oxidising agent
4 \(Z{n^{2 + }}\)is a reducing agent
Explanation:
(b)Since \(E_{Z{n^{ + + }}/Zn}^o\) is negative, so \(Zn\) has greater tendency to be oxidized than hydrogen. Hence it can act as reducing agent.
ELECTROCHEMISTRY
20085
\(2{H^ + }\,(aq) + 2{e^ - }\, \to \,{H_2}\,(g).\)The standard electrode potential for the above reaction is (in volts)
1 \(0\)
2 \(+1\)
3 \(-1\)
4 None of these
Explanation:
(a)Standard electrode potential of Hydrogen is zero.
ELECTROCHEMISTRY
20086
\(K,\,\,Ca\) and \(Li\) metals may be arranged in the decreasing order of their standard electrode potentials as
1 \(K,\,\,Ca,\,\,Li\)
2 \(Ca,\,\,K,\,\,Li\)
3 \(Li,\,\,Ca,\,\,K\)
4 \(Ca,\,\,Li,\,\,K\)
Explanation:
(b)According to electrochemical series.
ELECTROCHEMISTRY
20087
The correct order of chemical reactivity with water according to electrochemical series
1 \(K > Mg > Zn > Cu\)
2 \(Mg > Zn > Cu > K\)
3 \(K > Zn > Mg > Cu\)
4 \(Cu > Zn > Mg > K\)
Explanation:
(a)The standard reduction potential of \({K^ + }\), \(M{g^{2 + }},\,\,\,Z{n^{ + 2}}\,\,C{u^{2 + }}\) increase in this order.
20083
When a rod of metal \(A\) is dipped in an aqueous solution of metal \(B\) (concentration of \({B^{2 + }}\) ion being \(1\,M\) ) at \({25\,^o}C\), the standard electrode potentials are \({A^{2 + }}/A\) \( = -0.76 \) volts, \({B^{2 + }}\) \(/B = + 0.34\) volts
1 \(A\) will gradually dissolve
2 \(B\) will deposit on \(A\)
3 No reaction will occur
4 Water will decompose into \({H_2}\) and \({O_2}\)
Explanation:
(b)Since \(E_{{A^{2 + }}/A}^o < E_{{B^{2 + }}/B}^o\). A has greater tendency to be oxidized. \(A + {B^{2 + }} \to {A^{2 + }} + B\).
ELECTROCHEMISTRY
20084
The reaction \(Z{n^{2 + }} + 2{e^ - } \to Zn\) has a standard potential of \( - 0.76\,V\). This means
1 \(Zn\) can't replace hydrogen from acids
2 \(Zn\) is a reducing agent
3 \(Zn\) is a oxidising agent
4 \(Z{n^{2 + }}\)is a reducing agent
Explanation:
(b)Since \(E_{Z{n^{ + + }}/Zn}^o\) is negative, so \(Zn\) has greater tendency to be oxidized than hydrogen. Hence it can act as reducing agent.
ELECTROCHEMISTRY
20085
\(2{H^ + }\,(aq) + 2{e^ - }\, \to \,{H_2}\,(g).\)The standard electrode potential for the above reaction is (in volts)
1 \(0\)
2 \(+1\)
3 \(-1\)
4 None of these
Explanation:
(a)Standard electrode potential of Hydrogen is zero.
ELECTROCHEMISTRY
20086
\(K,\,\,Ca\) and \(Li\) metals may be arranged in the decreasing order of their standard electrode potentials as
1 \(K,\,\,Ca,\,\,Li\)
2 \(Ca,\,\,K,\,\,Li\)
3 \(Li,\,\,Ca,\,\,K\)
4 \(Ca,\,\,Li,\,\,K\)
Explanation:
(b)According to electrochemical series.
ELECTROCHEMISTRY
20087
The correct order of chemical reactivity with water according to electrochemical series
1 \(K > Mg > Zn > Cu\)
2 \(Mg > Zn > Cu > K\)
3 \(K > Zn > Mg > Cu\)
4 \(Cu > Zn > Mg > K\)
Explanation:
(a)The standard reduction potential of \({K^ + }\), \(M{g^{2 + }},\,\,\,Z{n^{ + 2}}\,\,C{u^{2 + }}\) increase in this order.
20083
When a rod of metal \(A\) is dipped in an aqueous solution of metal \(B\) (concentration of \({B^{2 + }}\) ion being \(1\,M\) ) at \({25\,^o}C\), the standard electrode potentials are \({A^{2 + }}/A\) \( = -0.76 \) volts, \({B^{2 + }}\) \(/B = + 0.34\) volts
1 \(A\) will gradually dissolve
2 \(B\) will deposit on \(A\)
3 No reaction will occur
4 Water will decompose into \({H_2}\) and \({O_2}\)
Explanation:
(b)Since \(E_{{A^{2 + }}/A}^o < E_{{B^{2 + }}/B}^o\). A has greater tendency to be oxidized. \(A + {B^{2 + }} \to {A^{2 + }} + B\).
ELECTROCHEMISTRY
20084
The reaction \(Z{n^{2 + }} + 2{e^ - } \to Zn\) has a standard potential of \( - 0.76\,V\). This means
1 \(Zn\) can't replace hydrogen from acids
2 \(Zn\) is a reducing agent
3 \(Zn\) is a oxidising agent
4 \(Z{n^{2 + }}\)is a reducing agent
Explanation:
(b)Since \(E_{Z{n^{ + + }}/Zn}^o\) is negative, so \(Zn\) has greater tendency to be oxidized than hydrogen. Hence it can act as reducing agent.
ELECTROCHEMISTRY
20085
\(2{H^ + }\,(aq) + 2{e^ - }\, \to \,{H_2}\,(g).\)The standard electrode potential for the above reaction is (in volts)
1 \(0\)
2 \(+1\)
3 \(-1\)
4 None of these
Explanation:
(a)Standard electrode potential of Hydrogen is zero.
ELECTROCHEMISTRY
20086
\(K,\,\,Ca\) and \(Li\) metals may be arranged in the decreasing order of their standard electrode potentials as
1 \(K,\,\,Ca,\,\,Li\)
2 \(Ca,\,\,K,\,\,Li\)
3 \(Li,\,\,Ca,\,\,K\)
4 \(Ca,\,\,Li,\,\,K\)
Explanation:
(b)According to electrochemical series.
ELECTROCHEMISTRY
20087
The correct order of chemical reactivity with water according to electrochemical series
1 \(K > Mg > Zn > Cu\)
2 \(Mg > Zn > Cu > K\)
3 \(K > Zn > Mg > Cu\)
4 \(Cu > Zn > Mg > K\)
Explanation:
(a)The standard reduction potential of \({K^ + }\), \(M{g^{2 + }},\,\,\,Z{n^{ + 2}}\,\,C{u^{2 + }}\) increase in this order.
20083
When a rod of metal \(A\) is dipped in an aqueous solution of metal \(B\) (concentration of \({B^{2 + }}\) ion being \(1\,M\) ) at \({25\,^o}C\), the standard electrode potentials are \({A^{2 + }}/A\) \( = -0.76 \) volts, \({B^{2 + }}\) \(/B = + 0.34\) volts
1 \(A\) will gradually dissolve
2 \(B\) will deposit on \(A\)
3 No reaction will occur
4 Water will decompose into \({H_2}\) and \({O_2}\)
Explanation:
(b)Since \(E_{{A^{2 + }}/A}^o < E_{{B^{2 + }}/B}^o\). A has greater tendency to be oxidized. \(A + {B^{2 + }} \to {A^{2 + }} + B\).
ELECTROCHEMISTRY
20084
The reaction \(Z{n^{2 + }} + 2{e^ - } \to Zn\) has a standard potential of \( - 0.76\,V\). This means
1 \(Zn\) can't replace hydrogen from acids
2 \(Zn\) is a reducing agent
3 \(Zn\) is a oxidising agent
4 \(Z{n^{2 + }}\)is a reducing agent
Explanation:
(b)Since \(E_{Z{n^{ + + }}/Zn}^o\) is negative, so \(Zn\) has greater tendency to be oxidized than hydrogen. Hence it can act as reducing agent.
ELECTROCHEMISTRY
20085
\(2{H^ + }\,(aq) + 2{e^ - }\, \to \,{H_2}\,(g).\)The standard electrode potential for the above reaction is (in volts)
1 \(0\)
2 \(+1\)
3 \(-1\)
4 None of these
Explanation:
(a)Standard electrode potential of Hydrogen is zero.
ELECTROCHEMISTRY
20086
\(K,\,\,Ca\) and \(Li\) metals may be arranged in the decreasing order of their standard electrode potentials as
1 \(K,\,\,Ca,\,\,Li\)
2 \(Ca,\,\,K,\,\,Li\)
3 \(Li,\,\,Ca,\,\,K\)
4 \(Ca,\,\,Li,\,\,K\)
Explanation:
(b)According to electrochemical series.
ELECTROCHEMISTRY
20087
The correct order of chemical reactivity with water according to electrochemical series
1 \(K > Mg > Zn > Cu\)
2 \(Mg > Zn > Cu > K\)
3 \(K > Zn > Mg > Cu\)
4 \(Cu > Zn > Mg > K\)
Explanation:
(a)The standard reduction potential of \({K^ + }\), \(M{g^{2 + }},\,\,\,Z{n^{ + 2}}\,\,C{u^{2 + }}\) increase in this order.
