
8) Calculate the cell potential for the following reaction that takes place in an electrochemical cell...
8) Calculate the cell potential for the following reaction that takes place in an electro chemical cell at 25°C. Al(s) A13+(aq, 0.115 M)I I Al3+(aq, 3.89 M) | Al(s) A13+(aq)+3 e Al(s) Eo =-1.66 V A) 0030 V B) 0.090 V 91.66 V D) 0.00 V E) 0.060 V
1)Calculate the cell potential for the following reaction that
takes place in an electrochemical cell at 25°C.
Al(s) Al3+(aq, 0.115 M) Al3+(aq, 3.89 M) Al(s)
Question options: a) +0.090 V b)+1.66 V c)+0.030 V d)+0.060 V
e)0.00 V
2) Determine the identity of the daughter nuclide from the
positron emission of F.
Question options:
a)
N
b)
Na
c)
Ne
d)
O
e)
F
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) II Ag+(aq, 0.55 M)1 Ag(s) Sn2+ (aq) + 2 e Ag+ (aq) + e- Sn(s) Ag(s) E = -0.14 V E = 0.80 V -0.84 V +0.86 V 0 -0.93 V +1.12 V O 0.92 V
Calculate the cell potential (E cell) for the following reaction that takes place in an electrochemical cell at 25 ^C. 2 ClO2 (g) + Zn (s) ---> 2 ClO2 (aq) + Zn^2+ (aq) [Zn^2+]=0.46 M, P-ClO2=0.015 atm, [ClO2]=0.75 M ClO2 (g) + e- ----> ClO2^- (aq) E^o= 0.95 V
Consider the following electrochemical cell: Al (s) I Al3+ (aq) (1.00 M) II Cu2+ (aq) (0.0020 M) I Cu (s) where Cu2+ aq + 2e- -> Cu (s) +0.34 V and Al3+ aq + 3e- -> Al (s) -1.66 V Calculate the standard cell potential for the given cell, calculate the cell potential for the given cell, and sketch the electrochemical cell using two beakers and labeling the electrodes, the cathode, the anode, the direction of electron flow in the...
Use measured cell potential to calculate concentration. When [ Hg2+ ]=1.35 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.582 V. What is the Al** concentration in this cell? 3 Hg2+ (aq) + 2 Al (s) — 3 Hg (1) + 2 A1+ (aq) [A13+]= M
For the reaction I2(s) + Cu(s) ↔ Cu2+(aq) + 2I-(aq) The following electrochemical cell is made: Cu(s)|Cu2+(aq, 0.1 M)||I‐(aq, 0.1 M)|I2(s)|C(s) At 25 C the cell potential for the above cell was measured and found to be 0.279 V. Calculate E°cel
22) Given the following redox reaction conducted in an acidic electrochemical cell, calculate ΔG®, ΔG, Eocell, and Ecell using the conditions provided. Al (s)VO2 (aq)Al (aqVo2 (aq) VO2(a)2H (aq)e VO2(a)H20() E 1.00V Al3+(aq) + 3e - Al (s) Eo 1.66V [VO2]- 1.2M [Al+0.025M vo21 0.05M [H ] 2.1M
22) Given the following redox reaction conducted in an acidic electrochemical cell, calculate ΔG®, ΔG, Eocell, and Ecell using the conditions provided. Al (s)VO2 (aq)Al (aqVo2 (aq) VO2(a)2H (aq)e VO2(a)H20() E 1.00V...
Given the following redox reaction conducted in an acidic electrochemical cell, calculate ΔGo, ΔG, Eocell, and Ecell using the conditions provided. Al (s) + VO2+ (aq) → Al3+ (aq) + VO2+ (aq) VO2+(aq) + 2H+(aq) + e- → VO2+(aq) + H2O(l) Eo = 1.00V Al3+(aq) + 3e- → Al (s) Eo = -1.66V [VO2+] = 1.2M [Al3+] = 0.025M [VO2+] = 0.05M [H+] = 2.1M
use tabulated standard electrode potential to calculate the
standard cell potential for the reaction occurring in an
electrochemical cell at 25 C. (The equation is balanced.)
3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq)
Express your answer to two significant figures and include the
appropriate units.
em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...