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Using the standard potential values give...

Using the standard potential values given below, decide which of the statements P,Q,R,S are correct?
Choose the right answer from (a), (b), (c ) and (d).
`Fe^(2+) + 2e^(-) rightarrow Fe`, `E^(@) = -0.44V`
`Cu^(2+) + 2e^(-) rightarrow Cu`, `E^(@) = +0.34V`
`Ag^(+) + e^(-) rightarrow Ag`, `E^(@) = +0.80V`
(P) Copper can displace iron from `FeSO_(4)` solution
(Q) Iron can displace copper from `CuSO_(4)` solution
(S) Iron can displace silver from `AgNO_(3)` solution

A

P and Q

B

Q and R

C

Q and S

D

P and S

Text Solution

Verified by Experts

The correct Answer is:
C
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Using the standard electrode potential values given below, decide which of the statements, I,II,III and IV are correct. Choose the right answer from (1) (2) and (4) Fe^(2+)+2e^(-) hArr " "," "E^(0)=-0.44V Cu^(2+)+2e^(-) hArr Cu" "," "E^(0)=+0.34V Ag^(+)+e^(-)hArr Fe" "," "E^(0)=+0.80V I. Copper can displace iron from FeSO_(4) solution. II. Iron can displace copper from CuSO_(4) solution III. Silver can displace copper from CuSO_(4) solution IV. Iron can displace silver from AgNO_(3) solution.

Cu^(+) + e^(-) rightarrow Cu , E^(@) = x1volt , Cu^(2+) + 2e^(-) rightarrow Cu , E^(@) = x_(2) volt, then for Cu^(2+) + e^(-) rightarrow Cu^(+), E^(@) (volt) will be :

Given the standard reduction potentials, which statement is correct? {:(Cu^(2)(aq) + 2e^(-) rightarrow Cu(s), E^(@) = 0.34V), (2H^(+)(aq) + 2e^(-) rightarrow H_(2)(g), E^(@)= 0.0V), (Cr^(3+)(aq) + 2e^(-) rightarrow Cr(s),E^(@) = -0.73V):}

Which of the half reactions, when coupled, will make a galvanic cell that will produce the largest voltage under standard conditons? P. Cu^(2+)(aq) + 2e^(-) rightarrow Cu(s) E^(@) = +0.34V Q. Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V R. Ag^(+)(aq) + 3e^(-) rightarrow Al(s) E^(@) = -1.66V

Given : Hg_(2)^(2+) +2 e ^(-)rightarrow 2Hg , E^(@) = 0.789 V and Hg^(2+) + 2e^(-) rightarrow Hg , E^(@) = 0.854V Calculate the equilibrium consant for Hg_(2)^(2+) rightarrow Hg + Hg^(2+) .

According to the reductions potentials in the table below, which statements is true under standard conditions? {:("Reaction", E^(@)V), (L^(2+) + 2e^(-) rightarrow L, -0.13), (M^(2+) + 2e^(-) rightarrow M, -0.44),(N^(2+) + 2e^(-) rightarrow N, -0.76):}

Given these standard reduction potentials, what is the standard reduction potential for Co^(3+)(aq) + 3e^(-) rightarrow Co(s) ? Co^(3+)(aq) + e^(-) rightarrow Co^(2+)(aq) E^(@) = 1.82V Co^(2+)(aq) + 2e^(-) rightarrow Co(s) E^(@) = -0.28V

Given these standards reduction potentials, what is the free energy change (in kJ. Mol^(-) for the reaction: Pb(s) + 2Ag^(+)(aq) rightarrow Pb^(2+)(aq) + 2Ag(s) Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.80V Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V

For a galvanic cell involving the half-reaction at standard conditions, Au^(3+) + 3e(-) rightarrow Au E^(@) = 1.50V Tl^(+) + e(-) rightarrow Tl E^(@) = -0.34V

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