Compute E0 for the process ZnY2- + 2e- = Zn(s) + Y4- where Y4- is the...

Compute E0 for the process ZnY2- + 2e- = Zn(s) + Y4- where Y4- is the completely deprotonated anion of EDTA. The formation constant for ZnY2- is 3.2x1016.

Expert Solution

Amanda K answered 6 months ago

Given the E0 values of the following two half-reactions: Zn à Zn2+ + 2e- E0 =...

Given the E0 values of the following two half-reactions: Zn à Zn2+ + 2e- E0 = 0.763 volt Fe à Fe2+ + 2e- E0 = 0.441 volt a)Write a balanced complete oxidation-reduction reaction? b)Explain whether the corrosion of an iron pipe (i.e., Fe Fe2+) in the presence of Zn/Zn2+ is possible or not (thermodynamically)? c)Explain whether or not Zn will protect the corrosion of iron pipe if metallic Zn is in contact with the iron pipe?

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq)...

Using the following reduction potentials: I2(s) + 2e- <---> 2I-(aq) E0 = 0.535 V I2 (aq) +2e- <---> 2I-(aq) E0 = 0.620 V I3-(aq) + 2e- <---> 3I-(aq) E0 = 0.535 V a) Calculate the equilibrium constant for I2(aq) + I-(aq) <---> I3-(aq) b) Calculate the equilibrium constant for I2(s) + I-(aq) <---> I3-(aq) c) Calculate the solubility (g/L) of I2(s) in water.

a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V

13)) a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will F-(aq) reduce Zn2+(aq) to Zn(s)? (6) Which species can be reduced by H2(g)? If none, leave box blank. b)) Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +...

complete and balance the net ionic equations for reactions that would occur: Zn(s)+Mg2+(aq)---> Zn(s)+Cu2+(aq)----> Zn(s)+H+(aq)-----> Mg(s)+Zn2+(aq)----->...

complete and balance the net ionic equations for reactions that would occur: Zn(s)+Mg2+(aq)---> Zn(s)+Cu2+(aq)----> Zn(s)+H+(aq)-----> Mg(s)+Zn2+(aq)-----> Mg(s)+Cu2+(aq)---> Mg(s)+H+(aq)----> Cu(s)+Zn2+(aq)----> Cu(s)+Mg2+(aq)----> Cu(s)+H+(aq)----->

The chemical reactions: CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) Zn(s) + H2SO4(aq) → ZnSO4(aq) +...

The chemical reactions: CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) The copper on the surface quickly reacts with oxygen according to the following reaction: 2Cu(s) + O2(g) → 2CuO(s) Experimental Procedure Dissolve completely about 0.5 to 0.7 g of copper (II) sulphate pentahydrate in about 10 to 20 mL of deionized water. Calculate the amount of zinc powder that must be added to a copper sulfate solution so that the sulfate completely reacts....

Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for...

Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for this voltaic cell. c) Calculate the cell potential for this voltaic cell at 298 K if it is constructed using solutions of 0.14 M Co(NO3)2 and 0.27 M Fe(NO3)2. d) When looking at the magnitude of this potential, what can be concluded about the electrochemical cell?

Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45...

Reduction half-reaction E∘ (V) Ag+(aq)+e−→Ag(s) 0.80 Cu2+(aq)+2e−→Cu(s) 0.34 Sn4+(aq)+4e−→Sn(s) 0.15 2H+(aq)+2e−→H2(g) 0 Ni2+(aq)+2e−→Ni(s) −0.26 Fe2+(aq)+2e−→Fe(s) −0.45 Zn2+(aq)+2e−→Zn(s) −0.76 Al3+(aq)+3e−→Al(s) −1.66 Mg2+(aq)+2e−→Mg(s) −2.37 1) Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) 2) Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 3.80×10−4. Express your answer to three significant figures and include the appropriate units.

A Zn-Cu battery is constructed as follows at 25oC Zn(s) | Zn+2(aq) (0.20 M) || Cu+2(aq)...

A Zn-Cu battery is constructed as follows at 25oC Zn(s) | Zn+2(aq) (0.20 M) || Cu+2(aq) (2.5 M) | Cu(s) The mass of each electrode is 200.0 gram and the volume of the electrolytes is 1.0 L a) calculate the cell potential of the cell b) calculate the mass of each electrode after 10.0 amp. of current has flowed for 10.0 hour Remember, the anode loses mass because of the oxidation reaction while the cathode gains mass due to the...

Concerning the reaction: 2 HCl(aq) + Zn(s)  H2(g) + ZnCl2(aq) A piece of Zn with...

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Calculate E at 25° C for a galvanic cell based on the reaction: Zn(s) + Cu2+(aq)→Zn...

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