3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s)...
3. Consider the following electrochemical cell. Standard
reduction potentials are given on the next page.
Tl(s) | Tl+(aq, 0.50 mol L−1) || H+(aq, x mol L−1) | H2(g, 1 atm) |
Pt(s)
The concentration of H+ is unknown and the pressure of H2 is kept
constant at 1 atm. The cell voltage is initially measured as 0.139
V, with the Pt | H2 | H+ half-cell acting as the cathode.
(a) (6 marks) Write out the oxidation and reduction half reactions,
and overall chemical reaction occurring in this electrochemical
cell. What is the initial pH in the Pt | H+ | H2 half-cell?
(b) (3 marks) What is the value of the equilibrium constant for the
reaction occurring in this cell?
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3. Consider the following electrochemical cell. Standard
reduction potentials are given on the next page.
Tl(s)...
given this electrochemical cell: Concentration of H+ is unknown, Pressure of H2 is constant at 1...
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
♡ Search this course Faded 0 x cell potentials given below. Standard Reduction Potentials (Volts) at...
♡ Search this course Faded 0 x cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C 12() + 2 6 2 I'(aq) 0.535 02(g) + 4 Hz0+ (aq) + 4 € -6 H,00 1.229 2 H2O(l) + 2 € H2(g) + 2 OH"(aq) -0.828 Sc3(aq) + 3 e Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: Se*(aq) + 3 6 —- Sc(S) -2.080|| Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential?
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │...
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M a. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each. b. Determine what reaction occurs overall, and calculate the Eo cell for this electrochemical cell. c. Make a drawing of this cell, and label the ANODE and the CATHODE....
Given the following standard reduction potentials: Tl(3+) + e(-) ---> Tl(2+) E°= -0.37 V Tl(3+) +...
Given the following standard reduction potentials: Tl(3+) + e(-) ---> Tl(2+) E°= -0.37 V Tl(3+) + 2e(-) ---> Tl(+) E°= 1.25 V (a) Calculate the half-cell potential for the half-reaction Tl(2+) + e(-) ---> Tl(+) (b) Determine of the following disproportionate reaction will occur sponta- neously in aqueous solution in the standard condition. 2Tl(2+)(aq) ---> Tl(3+)(aq) + Tl(+)(aq)
Use the standard reduction potentials to determine the G of the reaction of Tl(s) and H(aq)...
Use the standard reduction potentials to determine the G of the
reaction of Tl(s) and H(aq) to produce (a) Tl(aq) and H2(g) and (b)
Tl5+(aq) and H2(g).
14.27 Use standard reduction potentials to determine the Δ Go of the reaction of Tl (s) and H' (ag) to produce (a) TI (ag) and H2(g) and (b) TI3 (aa) and H2(g). Which reaction is more thermodynamically spontaneous under standard-state condi- tions? Comment on the results relative to the incrt-pair effect.
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1...
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1 atm) /Pt Given the following standard reduction potentials: Reaction 2 H+ (aq) + 2 Cd + (aq) + 2e H2 (aq) Cd (s) Eº (volts) 0.00 -0.40 (a) Write the equation for the overall cell reaction. (b) Calculate E' for the overall reaction. (c) Calculate the equilibrium constant for the overall reaction. (d) Calculate the actual value of E for the cell at the...
Use standard reduction potentials to determine the ∆G0 of the reaction of Tl(S) and H+(aq) to...
Use standard reduction potentials to determine the ∆G0 of the reaction of Tl(S) and H+(aq) to produce (a) Tl+(aq) and H2(g)and (b) Tl3+(aq) and H2(g). Which reaction is more thermodynamically spontaneous under standard-state conditions? Comment on the results relative to the inert-pair effect.
A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard...
A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: 2Fe3+(aq) + Pb(s) ---> 2Fe2+(aq) + Pb2+(aq) Answer: ____ kJ K for this reaction would be ________ (greater/less) than one. B) The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.12 M and [H+] = 6.80×10-3 M, is -178 kJ: Hg2+(1.12 M) + H2(g) ---> Hg(l) + 2H+(6.80×10-3 M) ΔG =...
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode...
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt($)|H2(9, 1.0 bar) H+ (aq, 1.0 mol L-Aus+ (aq,? mol L-)|Au(s). Part A What is the concentration of Au3+ in the solution if Ecell is 1.23 V ? Express your answer using two significant figures. YO ALC * * O O ? Au3+1 = mol L-1 Submit Request Answer
For the electrochemical cell below, the half-cell on the left is the anode and the cell...
For the electrochemical cell below, the half-cell on the left is the anode and the cell potential is 0.183 V at 25 °C. What is the concentration of H+, x, in mol L-1? Note: The symbol M is an abbreviation for mol L-1. Pt(s) | V2*(aq, 0.620 M), va(aq, 0.650 M) || H'(aq, xM) | H2(g, 1.30 bar) Pt(s) Half reaction 2 H(aq) 2eH2(g) V(a)V(aq) Eo V 0.000 -0.255 Enter a value accurate to 3 significant figures. x-[H]Number mol L-1
given this electrochemical cell:
Concentration of H+ is unknown, Pressure of H2 is constant at 1
atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+
half-cell acting as the cathode.
a) write out the oxidization and reduction half reactions, and
the overall chemical reaction occurring, and find the initial pH in
the H+ | H2 | Pt cell
b) What is the equilibrium constant of the reaction happening in
the cell?
Tl(s) | Tl*(aq, 0.50 mol...
♡ Search this course Faded 0 x cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C 12() + 2 6 2 I'(aq) 0.535 02(g) + 4 Hz0+ (aq) + 4 € -6 H,00 1.229 2 H2O(l) + 2 € H2(g) + 2 OH"(aq) -0.828 Sc3(aq) + 3 e Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: Se*(aq) + 3 6 —- Sc(S) -2.080|| Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential?
Use the standard reduction potentials to determine the G of the
reaction of Tl(s) and H(aq) to produce (a) Tl(aq) and H2(g) and (b)
Tl5+(aq) and H2(g).
14.27 Use standard reduction potentials to determine the Δ Go of the reaction of Tl (s) and H' (ag) to produce (a) TI (ag) and H2(g) and (b) TI3 (aa) and H2(g). Which reaction is more thermodynamically spontaneous under standard-state condi- tions? Comment on the results relative to the incrt-pair effect.
8. Consider the following electrochemical cell: Cd Cd? (0.20 M) // H (0.05 M), H2 (1 atm) /Pt Given the following standard reduction potentials: Reaction 2 H+ (aq) + 2 Cd + (aq) + 2e H2 (aq) Cd (s) Eº (volts) 0.00 -0.40 (a) Write the equation for the overall cell reaction. (b) Calculate E' for the overall reaction. (c) Calculate the equilibrium constant for the overall reaction. (d) Calculate the actual value of E for the cell at the...
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt($)|H2(9, 1.0 bar) H+ (aq, 1.0 mol L-Aus+ (aq,? mol L-)|Au(s). Part A What is the concentration of Au3+ in the solution if Ecell is 1.23 V ? Express your answer using two significant figures. YO ALC * * O O ? Au3+1 = mol L-1 Submit Request Answer
For the electrochemical cell below, the half-cell on the left is the anode and the cell potential is 0.183 V at 25 °C. What is the concentration of H+, x, in mol L-1? Note: The symbol M is an abbreviation for mol L-1. Pt(s) | V2*(aq, 0.620 M), va(aq, 0.650 M) || H'(aq, xM) | H2(g, 1.30 bar) Pt(s) Half reaction 2 H(aq) 2eH2(g) V(a)V(aq) Eo V 0.000 -0.255 Enter a value accurate to 3 significant figures. x-[H]Number mol L-1
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