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22) Given the following redox reaction conducted in an acidic electrochemical cell, calculate ΔG®...
Given the following redox reaction conducted in an acidic electrochemical cell, calculate ΔGo, ΔG, Eocell, and...
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
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...
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...
Using the equation: ΔG° = -nFE°cell calculate ΔG° and indicate if the reaction below is spontaneous...
Using the equation: ΔG° = -nFE°cell calculate ΔG° and indicate if the reaction below is spontaneous or non spontaneous: Al(s) | Al3+ (0.0020 M) | | Cu2+ (0.10 M) | Cu(s) The reduction potentials for the half reactions are Al3+(aq) + 3e- --> Al(s) = -1.662 V Cu2+(aq) +2e- --> Cu(s) = +0.3419 V
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 electrochemical cell at 25°C. 8) 10 Al(s) Al3+(aq, 0.1 15 M) I Al3 (aq, 3.89 M) I Al(s) A13+(aq)+3 e Al(s) E =-1.66 V A) 0,030 V B) 0.090 V 9,1.66 V D) 0.00 V E) 0.060 V
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
1)Calculate the cell potential for the following reaction that takes place in an electrochemical cell at...
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
Answer the following questions related to the given electrochemical cell. Answer the following questions related to...
Answer the following questions related to the given
electrochemical cell.
Answer the following questions related to the given electrochemical cell 2NO(g) H20(l) 2e N20(g) 20H (aq) 0.760 V NO aq) H2O(l) 2e NO2 (aq) 20H (aq) Eo 0.010 V 1. Answer the following questions under standard conditions (a) The half cell containing N20/NO is the (b) The half cell containing NO3 /NO2 s the (c) What is Eocell (in V)? Report your answer to three decimal places in standard notation...
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M...
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M and [Mn2+] = 0.30 M. 2 Al(s) + 3 Mn2+(aq) + 2 A13+(aq) + 3 Mn(s) Ecell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (cell) at 298 K. n= (Select] Q = (Select] Ecell = (Select)
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq)...
1.) Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s), what is the balanced overall (net) cell reaction? A. H2(g) + 2Ag(s) ® H+(aq) + 2Ag+(aq B. H2(g) + 2Ag+(aq) ® 2H+(aq) + 2Ag(s) C. H2(g) + Ag+(aq) ® H+(aq) + Ag(s D. 2H+(aq) + 2Ag(s) ® H2(g) + 2Ag+(aq) E. 2H+(aq) + 2Ag+(aq) ® H2(g) + 2Ag(s) 2.) Calculate E°cell for the following (nonspontaneous) reaction: Cd(s) + 2Fe3+(aq) ® 2Fe2+(aq) + Cd2+(aq) → A. -0.37...
Given the following result from balancing this redox reaction in acidic solution, carry on with the...
Given the following result from balancing this redox reaction in acidic solution, carry on with the last two steps to balance the redox reaction in basic solution. 2H+ (aq) + 2MnO4 (aq) + Br" (aq) → 2MnO2(3) + Br03 (aq) + H20(1) Once completed, choose the sum of the coefficients below: a) 7 b) 10 c) 13 d) 9 e) 12
8) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. 8) 10 Al(s) Al3+(aq, 0.1 15 M) I Al3 (aq, 3.89 M) I Al(s) A13+(aq)+3 e Al(s) E =-1.66 V A) 0,030 V B) 0.090 V 9,1.66 V D) 0.00 V E) 0.060 V
Answer the following questions related to the given
electrochemical cell.
Answer the following questions related to the given electrochemical cell 2NO(g) H20(l) 2e N20(g) 20H (aq) 0.760 V NO aq) H2O(l) 2e NO2 (aq) 20H (aq) Eo 0.010 V 1. Answer the following questions under standard conditions (a) The half cell containing N20/NO is the (b) The half cell containing NO3 /NO2 s the (c) What is Eocell (in V)? Report your answer to three decimal places in standard notation...
D Question 14 3 pts The following redox reaction is conducted with [A13+] = 0.80 M and [Mn2+] = 0.30 M. 2 Al(s) + 3 Mn2+(aq) + 2 A13+(aq) + 3 Mn(s) Ecell = 0.48 V Determine the moles of electrons transferred for the reaction as written (n), Q, and the cell potential (cell) at 298 K. n= (Select] Q = (Select] Ecell = (Select)
Given the following result from balancing this redox reaction in acidic solution, carry on with the last two steps to balance the redox reaction in basic solution. 2H+ (aq) + 2MnO4 (aq) + Br" (aq) → 2MnO2(3) + Br03 (aq) + H20(1) Once completed, choose the sum of the coefficients below: a) 7 b) 10 c) 13 d) 9 e) 12
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