For the following electrochemical cell:
Co(s)/Co^2+(aq,0.0155M)//Ag^+(aq,2.50M)/Ag(s)
Write the net equation:______________
Calculate the following values at 25 degrees celcius using the standard potentials:
E standard cell ________V
E cell _____________V
Ag+ + e-
Ag
Eo = +0.7996
Co
Co2+ +
e-
Eo = +0.28
----------------------
Ag+ + Co Ag +
Co2+ Eo = 0.7996 + 0.28 = 1.0796
V = E standard cell
Q = [Co2+]/[Ag+] = (0.0155)/(2.50) = 6.2
10-3
E = Eo - (0.0591/n)log Q
E = 1.0796 - (0.0591/2) log (6.2 10-3)
= 1.144 V = E cell
For the following electrochemical cell: Co(s)/Co^2+(aq,0.0155M)//Ag^+(aq,2.50M)/Ag(s) Write the net equation:______________ Calculate the following values at 25...
Write the net cell equation.
Calculate the following values at 25.0 degrees C
For the following electrochemical cell Cu(s)|Cu2+(aq, 0.01 55 M)IAg+(aq, 2.50 M)|Ag(s) write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25.0 °C using standard potentials as needed. Number Number kJ/ mol cell Number Number k.J/ mol
Write the net cell equation for this electrochemical cell.
Phases are optional. Do not include the concentrations.
Co(s)∣∣Co2+(aq, 0.0155 M)‖‖Ag+(aq, 2.50 M)∣∣Ag(s)Co(s)|Co2+(aq,
0.0155 M)‖Ag+(aq, 2.50 M)|Ag(s)
net cell equation:
Co+2Ag+⟶Co2++2AgCo+2Ag+⟶Co2++2Ag
Calculate ?∘cellEcell∘, Δ?∘rxnΔGrxn∘, Δ?rxnΔGrxn, and ?cellEcell
at 25.0 ∘C25.0 ∘C, using standard potentials as needed
Calculate Ecell, AGixn , AGxn , and Ecell at 25.0 °C, using standard potentials as needed. AG x = -89.4 AGxn = -104 E cell = .54
Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations. Cu(s) Cu2 (aq, 0.0155 M) || Agt (aq, 2.50 M)| Ag(s) net cell equation: Calculate E and Ecell at 25 C, using standard potentials as needed cell V cell Ecell V
For the following electrochemical cell Sn(s)|Sn?(aq, 0.0155 M)lAg (aq, 2.50 M)JAg(s) write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25.0 ℃ using standard potentials as needed Number Number kJ/ mol cell Number Number &Grin- kJ/ mol cell
Consider the following electrochemical cell shown below. Sn(s)|Sn2 (aq, 0.0155 M)lIAg (aq, 3.50 M)IAg(s) Based on this cell write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25 °C using standard potentials as needed. Number cell Number cell
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+ (aq, 0.50 M)||I^- (aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e^- rightarrow Ag(s) + I^-(aq) E degree = -0.15 V Sn^4+ (aq) + 2 e^- rightarrow SN^2+ (aq) E degree= +0.15 V.
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
The following electrochemical cell is being studied in an experiment: Cr (s) | Cr3+ (aq) || Cu2+ (aq) | Cu (s) A. Write the balanced equation for the overall reaction. (4pts) B. Calculate the value of Eo cell using standard reduction potentials. See Slide 21 in Ch. 20 images if needed. (4pts) C. Is this a voltaic or electrolytic cell? Explain briefly. (4pts) D. Which metal electrode will the electrons flow towards? (2pts) E. Calculate the value of Go, in...
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction and its standard cell potential (in V) at 25°C for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction (please provide)= standard cell potential V= Is the reaction spontaneous at standard conditions?
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V