Calculate the cell potential for the galvanic cell in which the following reaction occurs at 25...

Calculate the cell potential for the galvanic cell in which the following reaction occurs at 25 °C, given that [Al3 ] = 0.00120 M and [Au3 ] = 0.787 M.

Al (s) + Au^3+ (aq) <===> Al^3+ (aq) + Au (s)

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

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

Calculate E at 25° C for a galvanic cell based on the reaction: Zn(s) + Cu2+(aq)→Zn 2+(aq) + Cu (s) in which [Zn2+]=0.55M and [Cu2+]=1.02M

Calculate the cell potential for a reaction in a electrolytic cell with the following half-reactions if:...

Calculate the cell potential for a reaction in a electrolytic cell with the following half-reactions if: [U 3+] = 0.10 M, [MnO4 - ] = 0.20M, [Mn2+], and [H+ ] = 0.20 M U 3+ + 3e -> U o Ecell = - 1.642 V MnO4 - + 8H+ + 5e- -> Mn2+ + 4H2O Ecell = +1.51 V

The cell voltage for the following galvanic cell is 1.27V. Calculate the pH of the solution...

The cell voltage for the following galvanic cell is 1.27V. Calculate the pH of the solution at 25oC: 2Ag+(0.010 M) + H2(1 atm) → 2Ag(s) + 2H+(pH = ?)

For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half...

For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 in the Background as needed. Explain how you identified which half-reaction is the oxidizer and which is the reducer. Balance the equation. Show your work. (8pts) Al(s) + Ag+1(aq)à Ag(s) + Al+3(aq) Please type your answer out please

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2...

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.759 M and [Ni2 ] = 0.0120 M. Standard reduction potentials can be found here. Cr + Ni^2+ <----> Cr^2+ + Ni

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2...

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Cr2 ] = 0.884 M and [Fe2 ] = 0.0190 M. Standard reduction potentials can be found here. Cr(s) + Fe2+(aq) -> Cr2+(aq) + Fe(s)

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2...

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2 ] = 0.763 M and [Sn2 ] = 0.0140 M. Standard reduction potentials can be found here. Zn(s)+SN2+ YIELDS Zn2+(aq)+Sn(s)

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2...

Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.799 M and [Sn2 ] = 0.0160 M. Standard reduction potentials can be found here. Mg(s)+ Sn^2+ ---> Mg^2+ +Sn(s) E= V units

A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...

A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. 1.) [Fe3+]= 1.1×10−3 M ; [Mg2+]= 2.60 M 2.) [Fe3+]= 2.60 M ; [Mg2+]= 1.1×10−3 M

A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...

A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions a)[Fe3+]= 1.0×10−3 M ; [Mg2+]= 2.00 M b)[Fe3+]= 2.00 M ; [Mg2+]= 1.0×10−3 M

Subjects