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If E(Sn^(2+)//Sn)^(@)=-0.14V, what would...

If `E_(Sn^(2+)//Sn)^(@)=-0.14V,` what would be the value of `E_(Sn//Sn^(2+))^(@)`?

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To find the value of \( E^\circ_{Sn//Sn^{2+}} \) given \( E^\circ_{Sn^{2+}//Sn} = -0.14 \, V \), we can follow these steps: ### Step 1: Write the given half-reaction and its standard electrode potential We know that: \[ E^\circ_{Sn^{2+} + 2e^- \rightarrow Sn} = -0.14 \, V \] ...
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Consider the following E^@ values . E_(Fe^(3+)//Fe^(2+)^@ = + 0.77 V , E_(Sn^(2+)//Sn)^@=- 0.14 V The E_(cell)^@ for the reaction , Sn (s) + 2Fe^(3+)(aq) rarr 2 Fe^(2+)(aq)+ Sn^(2+)(aq) is ? (a) -0.58 V (b) -0.30 V (c) +0.30V (d) +0.58 V

A solution is 1 molar in each of NaCl, CdCl_(2), ZnCl_(2) and PbCl_(2) . To this Sn metal is added, which of the following is true? Given E^(@) (Pb^(2+)//Pb = -0.126V) E_(Sn^(2+)//Sn)^(@) = -0.136V, E_(Cd^(2+)//Cd)^(@) = -0.40V E_(Zn^(2+)//Zn)^(@) = -0.763V, E_(Na^(+)//Na)^(@)= -2.71V

Consider the following E^(@) values E^(@) values E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v , E_(Sn^(2+)//Sn)^(@) = -0.14 under standard condition the potential for the reaction Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq) is :

Select the correct statement if- E_(Mg^(2+)//Mg)^(@)=-2.4V, E_(Sn^(4+)//Sn^(2+))^(@)=0.1V, E_(MnO_(4)^(-),H^+//Mn^(2+))^(@)=1.5V, E_(I_(2)//I^(-))^(@)=0.5V

A half cell is prepared by K_(2)Cr_(2)O_(7) in a buffer solution of pH =1 . Concentration of K_(2)Cr_(2)O_(7) is 1M . To 3 litre of this solution 570 gm of SnCI_(2) is added which is oxidised completely to SnCI_(4) . Given: E_(Cr_(2)O_(7)^(-2)//Cr^(+3).H^(+))^(@) = 1.33V, (2.303)/(F) RT = 0.06 , Atomic of mass Sn = 119, E_(Sn^(+4)//Sn^(+2))^(@) = 0.15 Emf of the cell Pt|underset((0.1M))(Sn^(+2)),underset((0.2M))(Sn^(+4)),underset((1M))(H^(+)):||:underset((0.2M))(Cr_(2)O_(7)^(2-)),underset((1M))(Cr^(+3)),underset((1M))(H^(+)):|:Pt

Given: E_(Sn^(2+)//Sn) ^0 = -0.14V , E_(Pb^(2+)//Pb) ^0 = -0.13V . Determine [(Sn^(2+))//(Pb^(2+))] at equilibrium. For cell reaction Sn |Sn^(2+) || Pb^(2+) | Pb , Take (2.303RT)//F = 0.06V

Given: E_(Sn^(2+)//Sn) ^0 = -0.14V , E_(Pb^(2+)//Pb) ^0 = -0.13V . Determine [(Sn^(2+))//(Pb^(2+))] at equilibrium. For cell reaction Sn |Sn^(2+) || Pb^(2+) | Pb , Take (2.303RT)//F = 0.06V

A half cell is prepared by K_(2)Cr_(2)O_(7) in a buffer solution of pH =1 . Concentration of K_(2)Cr_(2)O_(7) is 1M . To 3 litre of this solution 570 gm of SnCI_(2) is added which is oxidised completely to SnCI_(4) . Given: E_(Cr_(2)O_(7)^(-2)//Cr^(+3).H^(+))^(@) = 1.33V, (2.303)/(F) RT = 0.06 , Atomic of mass Sn = 119, E_(Sn^(+4)//Sn^(+2))^(@) = 0.15 Half cell potential E_(Cr_(2)O_(7)^(-2)//Cr^(+3))^(@) after teh reaction of SnCI_(2) is:

Consider the following E^(@) values E^(o)""_(Fe^(3+)//Fe^(2+))= +0.77 V" "E^(o)""_(Sn^(2+)//Sn)= 0.14V Under standard conditions the EMF for the reaction Sn(s) + 2Fe^(3+) (aq) rarr 2Fe^(2+)(aq)+Sn^(2+)(aq) is :

Find the equilibrium constant of the following reaction Cu^(2+) (aq) +Sn^(2+) (aq) hArr Cu(s) +Sn^(4+) (aq) at 25^(@)C, E_(Cu^(2+)//Cu)^(Theta)=0.34V, E_(Sn^(4+)//Sn^(2+))^(Theta)=0.155V

ICSE-REDOX REACTIONS (OXIDATION AND REDUCTION)-VERY SHORT ANSWER TYPE QUESTIONS
  1. Write the half equations for each of the following redox reactions. ...

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  2. Write the half equations for each of the following redox reactions. ...

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  3. Name the type of reaction that occurs at anode in an electrochemical c...

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  4. What is the direction of flow of electrons in a galvanic cell?

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  5. In what form does chemical energy get converted when the oxidising and...

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  6. Define oxidation and reduction potentials.

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  7. If E(Sn^(2+)//Sn)^(@)=-0.14V, what would be the value of E(Sn//Sn^(2+)...

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  8. Define standard electrode potential.

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  9. The standard reduction potential for silver electrode is +0.80 V. It i...

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  10. E(Li^(+)//Li)^(@)=-3.05V and E(Ca^(2+)//Ca)^(@)=-2.87V, state which is...

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  11. Among Na and Mg, which is more reactive and why?

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  12. Write the cell reaction for each of the following cells. Pt,H(2)(g)|...

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  13. Write the cell reaction for each of the following cells. Ni(s)|Ni^(2...

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  14. In which direction the cell reaction would proceed if the E.M.F. of a ...

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  15. Represent the cell corresponding to the following redox reaction and i...

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  16. Write the Nernst equation at 298 K for the electrode reaction 2H^(+)...

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  17. Determine the oxidation number of the underlined elements in the follo...

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  18. Determine the oxidation number of C in the following: CO,CO(2),HCO(3...

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  19. Determine the oxidation number of O in the following: OF(2),Na(2)O(2...

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  20. Determine the change in the oxidation number of S in H(2)S and SO(2) i...

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