315403 The position of some metals in the electrochemical series in decreasing electropositive character is given as \(\mathrm{\mathrm{Mg}>\mathrm{Al}>}\) \(\mathrm{\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}}\). What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

315404 Zn gives \(\mathrm{\mathrm{H}_{2}}\) gas with \(\mathrm{\mathrm{H}_{2} \mathrm{SO}_{4}}\) and \(\mathrm{\mathrm{HCl}}\) but not with \(\mathrm{\mathrm{HNO}_{3}}\) because

315405 Consider the folowing reduction processes
\(\mathrm{Z n^{2+}+2 e \rightarrow Z n(S) ; E^{\circ}=-0.76 \mathrm{~V}}\)
\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2e}} \to {\rm{Ca}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{87}}\;{\rm{V}}\)
\({\rm{M}}{{\rm{g}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Mg}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{36}}\;{\rm{V}}\)
\({\rm{N}}{{\rm{i}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Ni}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{25}}\;{\rm{V}}\)
The reducing power of the metals increases inorder:

315406 The standard reduction potential at \(\mathrm{298 \mathrm{~K}}\) for the following half cell reaction:
\({\rm{Zn}}_{({\rm{aq}})}^{{\rm{2 + }}}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {\rm{Z}}{{\rm{n}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{762}}\;{\rm{V}}\)
\({\rm{Cr}}_{({\rm{aq}})}^{{\rm{3 + }}}{\rm{ + 3}}{{\rm{e}}^{\rm{ - }}} \to {\rm{C}}{{\rm{r}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{740}}\;{\rm{V}}\)
\({\rm{2H}}_{({\rm{aq}})}^{\rm{ + }}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {{\rm{H}}_{{\rm{2}}(\;{\rm{g}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{0}}\;{\rm{V}}\)
Which of the following is the strongest reducing agent?

315407 Assertion :
A metal having negative reduction potential when dipped in the solution of its own ions has a tendency to pass into the solution.
Reason :
Metal having negative reduction potential has large hydration energy.

315403 The position of some metals in the electrochemical series in decreasing electropositive character is given as \(\mathrm{\mathrm{Mg}>\mathrm{Al}>}\) \(\mathrm{\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}}\). What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

315404 Zn gives \(\mathrm{\mathrm{H}_{2}}\) gas with \(\mathrm{\mathrm{H}_{2} \mathrm{SO}_{4}}\) and \(\mathrm{\mathrm{HCl}}\) but not with \(\mathrm{\mathrm{HNO}_{3}}\) because

315405 Consider the folowing reduction processes
\(\mathrm{Z n^{2+}+2 e \rightarrow Z n(S) ; E^{\circ}=-0.76 \mathrm{~V}}\)
\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2e}} \to {\rm{Ca}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{87}}\;{\rm{V}}\)
\({\rm{M}}{{\rm{g}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Mg}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{36}}\;{\rm{V}}\)
\({\rm{N}}{{\rm{i}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Ni}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{25}}\;{\rm{V}}\)
The reducing power of the metals increases inorder:

315406 The standard reduction potential at \(\mathrm{298 \mathrm{~K}}\) for the following half cell reaction:
\({\rm{Zn}}_{({\rm{aq}})}^{{\rm{2 + }}}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {\rm{Z}}{{\rm{n}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{762}}\;{\rm{V}}\)
\({\rm{Cr}}_{({\rm{aq}})}^{{\rm{3 + }}}{\rm{ + 3}}{{\rm{e}}^{\rm{ - }}} \to {\rm{C}}{{\rm{r}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{740}}\;{\rm{V}}\)
\({\rm{2H}}_{({\rm{aq}})}^{\rm{ + }}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {{\rm{H}}_{{\rm{2}}(\;{\rm{g}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{0}}\;{\rm{V}}\)
Which of the following is the strongest reducing agent?

315407 Assertion :
A metal having negative reduction potential when dipped in the solution of its own ions has a tendency to pass into the solution.
Reason :
Metal having negative reduction potential has large hydration energy.

315403 The position of some metals in the electrochemical series in decreasing electropositive character is given as \(\mathrm{\mathrm{Mg}>\mathrm{Al}>}\) \(\mathrm{\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}}\). What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

315404 Zn gives \(\mathrm{\mathrm{H}_{2}}\) gas with \(\mathrm{\mathrm{H}_{2} \mathrm{SO}_{4}}\) and \(\mathrm{\mathrm{HCl}}\) but not with \(\mathrm{\mathrm{HNO}_{3}}\) because

315405 Consider the folowing reduction processes
\(\mathrm{Z n^{2+}+2 e \rightarrow Z n(S) ; E^{\circ}=-0.76 \mathrm{~V}}\)
\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2e}} \to {\rm{Ca}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{87}}\;{\rm{V}}\)
\({\rm{M}}{{\rm{g}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Mg}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{36}}\;{\rm{V}}\)
\({\rm{N}}{{\rm{i}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Ni}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{25}}\;{\rm{V}}\)
The reducing power of the metals increases inorder:

315406 The standard reduction potential at \(\mathrm{298 \mathrm{~K}}\) for the following half cell reaction:
\({\rm{Zn}}_{({\rm{aq}})}^{{\rm{2 + }}}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {\rm{Z}}{{\rm{n}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{762}}\;{\rm{V}}\)
\({\rm{Cr}}_{({\rm{aq}})}^{{\rm{3 + }}}{\rm{ + 3}}{{\rm{e}}^{\rm{ - }}} \to {\rm{C}}{{\rm{r}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{740}}\;{\rm{V}}\)
\({\rm{2H}}_{({\rm{aq}})}^{\rm{ + }}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {{\rm{H}}_{{\rm{2}}(\;{\rm{g}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{0}}\;{\rm{V}}\)
Which of the following is the strongest reducing agent?

315407 Assertion :
A metal having negative reduction potential when dipped in the solution of its own ions has a tendency to pass into the solution.
Reason :
Metal having negative reduction potential has large hydration energy.

315403 The position of some metals in the electrochemical series in decreasing electropositive character is given as \(\mathrm{\mathrm{Mg}>\mathrm{Al}>}\) \(\mathrm{\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}}\). What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

315404 Zn gives \(\mathrm{\mathrm{H}_{2}}\) gas with \(\mathrm{\mathrm{H}_{2} \mathrm{SO}_{4}}\) and \(\mathrm{\mathrm{HCl}}\) but not with \(\mathrm{\mathrm{HNO}_{3}}\) because

315405 Consider the folowing reduction processes
\(\mathrm{Z n^{2+}+2 e \rightarrow Z n(S) ; E^{\circ}=-0.76 \mathrm{~V}}\)
\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2e}} \to {\rm{Ca}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{87}}\;{\rm{V}}\)
\({\rm{M}}{{\rm{g}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Mg}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{36}}\;{\rm{V}}\)
\({\rm{N}}{{\rm{i}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Ni}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{25}}\;{\rm{V}}\)
The reducing power of the metals increases inorder:

315406 The standard reduction potential at \(\mathrm{298 \mathrm{~K}}\) for the following half cell reaction:
\({\rm{Zn}}_{({\rm{aq}})}^{{\rm{2 + }}}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {\rm{Z}}{{\rm{n}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{762}}\;{\rm{V}}\)
\({\rm{Cr}}_{({\rm{aq}})}^{{\rm{3 + }}}{\rm{ + 3}}{{\rm{e}}^{\rm{ - }}} \to {\rm{C}}{{\rm{r}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{740}}\;{\rm{V}}\)
\({\rm{2H}}_{({\rm{aq}})}^{\rm{ + }}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {{\rm{H}}_{{\rm{2}}(\;{\rm{g}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{0}}\;{\rm{V}}\)
Which of the following is the strongest reducing agent?

315407 Assertion :
A metal having negative reduction potential when dipped in the solution of its own ions has a tendency to pass into the solution.
Reason :
Metal having negative reduction potential has large hydration energy.

315403 The position of some metals in the electrochemical series in decreasing electropositive character is given as \(\mathrm{\mathrm{Mg}>\mathrm{Al}>}\) \(\mathrm{\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}}\). What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

315404 Zn gives \(\mathrm{\mathrm{H}_{2}}\) gas with \(\mathrm{\mathrm{H}_{2} \mathrm{SO}_{4}}\) and \(\mathrm{\mathrm{HCl}}\) but not with \(\mathrm{\mathrm{HNO}_{3}}\) because

315405 Consider the folowing reduction processes
\(\mathrm{Z n^{2+}+2 e \rightarrow Z n(S) ; E^{\circ}=-0.76 \mathrm{~V}}\)
\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2e}} \to {\rm{Ca}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{87}}\;{\rm{V}}\)
\({\rm{M}}{{\rm{g}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Mg}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 2}}.{\rm{36}}\;{\rm{V}}\)
\({\rm{N}}{{\rm{i}}^{{\rm{ + 2}}}}{\rm{ + 2e}} \to {\rm{Ni}}({\rm{s}});{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{25}}\;{\rm{V}}\)
The reducing power of the metals increases inorder:

315406 The standard reduction potential at \(\mathrm{298 \mathrm{~K}}\) for the following half cell reaction:
\({\rm{Zn}}_{({\rm{aq}})}^{{\rm{2 + }}}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {\rm{Z}}{{\rm{n}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = - 0}}.{\rm{762}}\;{\rm{V}}\)
\({\rm{Cr}}_{({\rm{aq}})}^{{\rm{3 + }}}{\rm{ + 3}}{{\rm{e}}^{\rm{ - }}} \to {\rm{C}}{{\rm{r}}_{({\rm{s}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{740}}\;{\rm{V}}\)
\({\rm{2H}}_{({\rm{aq}})}^{\rm{ + }}{\rm{ + 2}}{{\rm{e}}^{\rm{ - }}} \to {{\rm{H}}_{{\rm{2}}(\;{\rm{g}})}};{\rm{E}}^\circ {\rm{ = 0}}.{\rm{0}}\;{\rm{V}}\)
Which of the following is the strongest reducing agent?

315407 Assertion :
A metal having negative reduction potential when dipped in the solution of its own ions has a tendency to pass into the solution.
Reason :
Metal having negative reduction potential has large hydration energy.