Homework Answers
From the given reaction, we separate the half reactions and find out the number of electrons reacting in the reaction, which are common to both the half reactions. Then we substitute all the values in Nernst equation, which at 25°C becomes:
Ecell = E°cell - (0.0591/n)(log {[P]p/[R]r}).
The correct option on solving the Nernst equation comes out to be option (b). 0.44 V.
The detailed solution is given below:
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For the following electrochemical cell: 2 Al(s) + 3 Mn?"(aq) 2 Al3+ (aq) + 3 Mn(s)...
Consider the following electrochemical cell: Al (s) I Al3+ (aq) (1.00 M) II Cu2+ (aq) (0.0020...
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...
please help!!!! For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° =...
please help!!!!
For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s)...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
2. Write the cell notation for an electrochemical cell consisting of an anode where Mg (s)...
2. Write the cell notation for an electrochemical cell
consisting of an anode where Mg
(s) is oxidized to
Mg2+(aq) and a cathode
where Al3+(aq) is
reduced to Al (s) . Assume all
aqueous solutions have a concentration of 1 mol/L.
Enter electrons as e Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by...
Calculate e cell for the electrochemical cell below, Pb(s) |Pb2+(aq, 1.0 M) || Fe2+(aq, 1.0 M)...
Calculate e cell for the electrochemical cell below, Pb(s) |Pb2+(aq, 1.0 M) || Fe2+(aq, 1.0 M) | Fe(s) given the following reduction half-reactions. Pb2+(aq) + 2 e– ® Pb(s) E° = –0.126 V Fe2+(aq) + e– ® Fe(s) E° = –0.44 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
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)
For the electrochemical cell based on the following cell reaction: 2 F F2(g latm) + Mn(s)...
For the electrochemical cell based on the following cell reaction: 2 F F2(g latm) + Mn(s) (aq, 0.010M) + Mn²+(aq, 0.10M) Rxns Cathode E [V] F2(g) + 2 e + 2.87 2 F (aq) Mn²+(aq) + 2 - 1.18 e Mn(s) a) Determine E cell b) Determine E cell Ecell Ecell - RT/nF in Q
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) +...
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) + + OH (24) +1e UO2 (aq) +H2O Ered = -0.48 V Ti* (aq) + 1 e -Ti) Ered = -0.52 V a. Give the balanced net redox reaction in the spontaneous direction. (2 marks) b. What is Eºcell? (2 marks) c. In the working electrochemical cell applying the net redox reaction in the spontaneous direction under standard conditions of concentration, what material must the...
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
please help!!!!
For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...
3) A voltaic cell employs the following redox reaction: Sn2+ (aq) + Mn (s) →Sn (s) + Mn2+ (aq) a) Make a sketch of the cell. Label the cathode, anode, Sn2+, Mn, Sn, Mn?, and salt bridge. Indicate the direction of electron flow and the direction of ion flow from the salt bridge. b) Use line notation to represent the cell. c) What is the cell potential at 25°C when [Sn?] is 0.002 M and [Mn2+] is 0.050 M?
2. Write the cell notation for an electrochemical cell
consisting of an anode where Mg
(s) is oxidized to
Mg2+(aq) and a cathode
where Al3+(aq) is
reduced to Al (s) . Assume all
aqueous solutions have a concentration of 1 mol/L.
Enter electrons as e Use smallest possible integer coefficients for ALL reactions. If a box is not needed, leave it blank. A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by...
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
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)
For the electrochemical cell based on the following cell reaction: 2 F F2(g latm) + Mn(s) (aq, 0.010M) + Mn²+(aq, 0.10M) Rxns Cathode E [V] F2(g) + 2 e + 2.87 2 F (aq) Mn²+(aq) + 2 - 1.18 e Mn(s) a) Determine E cell b) Determine E cell Ecell Ecell - RT/nF in Q
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) + + OH (24) +1e UO2 (aq) +H2O Ered = -0.48 V Ti* (aq) + 1 e -Ti) Ered = -0.52 V a. Give the balanced net redox reaction in the spontaneous direction. (2 marks) b. What is Eºcell? (2 marks) c. In the working electrochemical cell applying the net redox reaction in the spontaneous direction under standard conditions of concentration, what material must the...
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