Using data found in Appendix E of your textbook calculate the
nonstandard emf for each of the following reactions if the
concentration of each of the ions in these reactions is 0.0007
molar and everything else is standard (use 298 K for the
temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol):
(a) 2 Li+(aq) + 1 Sn(s) --> 2 Li(s) + 1
Sn2+(aq)
(b) 1 Zn2+(aq) + 1 Ca(s) --> 1 Zn(s) + 1
Ca2+(aq)
(c) 1 Mg2+(aq) + 1 H2(g) --> 1 Mg(s) + 2
H+(aq)
(d) 2 Al3+(aq) + 3 Pb(s) --> 2 Al(s) + 3
Pb2+(aq)
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of...
33.Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 Hg2+(aq) + 1 Sn(s) --> 1 Hg22+(aq) + 1 Sn2+(aq) E = V (b) 1 Cd2+(aq) + 1 Sn2+(aq) --> 1 Cd(s) + 1 Sn4+(aq) E...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0003 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): 33. 0/0.1 points Previous Answers 1/4 Submissions Used My Notes Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0006 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 H+(aq) + 2 Cu(s) --> 1 H2(g) + 2 Cu+(aq) E = V (b) 1 Ca2+(aq) + 2 K(s) --> 1 Ca(s) + 2 K+(aq) E...
Part 1.) Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0002 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 2 Hg2+(aq) + 1 Sn(s) --> 1 Hg22+(aq) + 1 Sn2+(aq) E = __ V (b) 1 F2(g) + 1 Mg(s) --> 2 F-(aq)...
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions in these reactions is 0.0005 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the ions...
33 0.1 points 0/4 Submissions Used Using data found in Appendix E of your textbook caloulate the nonstandard emf for each of the following reactions if the concentration of each of the lons in these reactions is 0.0001 molar and everything else is standard (use 298K for the temperature, R 8.314 mol-K, and F 96,485 C/mol): My Notes (a) 1 Fala) + 1 Cus)->2 F (aq) +1 C(aq) E- (b) 2 Cu'(aq) 1 Fe(s)->2 Cu(s) + 1 Fe (a) E...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...
11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...