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Given these standards reduction potentia...

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`

A

-180

B

-90

C

90

D

180

Text Solution

Verified by Experts

The correct Answer is:
A
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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

Nickel metal is added to a solution containign 1.0 m Pb^(2+)(aq) and 1.0 M Cd^(2+)(aq) . Use the standard reduction potentials to determine which reaction(s) will occur. Reaction 1: Ni(s) + Pb^(2+)(aq) rightarrow Pb(s) + Ni^(2+)(aq) Reaction 2: Ni(s) + Cd^(2+)(aq) rightarrow Cd(s) + Ni^(2+)(aq) {:("Reaction", E^(@)), (Pb^(2+)(aq) + e^(-) rightarrow Pb(s) , -0.13V), (Ni^(2+)(aq) + 2e^(-) rightarrow Ni(s), -0.23V), (Cd^(2+)(aq) + 2e^(-) rightarrow Cd(s), -0.40V):}

Given the two standard reduction potentials below, what is the K_(sp) of Ag_(2)CrO_(4) at 25^(@)C ? Ag_(2)CrO^(4)(s) + 2e^(-) rightarrow 2Ag(s) + CrO_(4)^(2-)(aq) E^(@)= + 0.446V Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = +0.799V

Use the information in the table and calcualate E^(@) for this reaction. Ga(s) + 3Tl^(+)(aq) rightarrow 3Tl(s) + Ga^(3+) (aq) {: ("Reaction", E^(@)), (Ga^(3+)(aq) + 3e^(-) rightarrow Ga(s), -0.529V), (Tl^(+)(aq) + e^(-) rightarrow Tl(s), -0.336V):}

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):}

Use the standard reduction potentials to determine what is observed at the cathode during the electrolysis of a 1.0 M solution of KBr that contains phenolphthalein. O_(2)(g) + 4H^(+)(aq) + 4e^(-) rightarrow 2H_(2)O(l) E^(@) = 1.23V Br_(2)(l) + 2e^(-) rightarrow 2Br^(-)(aq) E^(@) = 1.07V 2H_(2)O(l) + 2e^(-) rightarrow H_(2)(g) + 2OH^(-) E^(@0 = -0.80V K^(+) (aq) + e^(-) rightarrow K(s) E^(@) = -2.92V

The equilibrium constent of the reaction. Cu(s)+2Ag(aq). Leftrightarrow Cu^(2+) (aq.)+2Ag(s) E^(@)=0.46" V at 298 K is"

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