Question 4: (a) What are redox reactions? Explain the difference between a gal-vanic and an electrolytic cell. Consider the cell described below:Al | AF (1.00M) | Pb²*(1.00M)| PbCalculate the cell potential after the reaction has operated long enough forthe [Al3+] to have changed by 0.60 mol/L. (Assume T = 25°C.)(h) Many elementa hau

In certain reactions, transfer of electrons takes place from one species to another. There are two…

Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP*(1.00M) || Pb²*(1.00M) | Calculate the cell potential after the reaction has operated long enough for the [Al3+] to have changed by 0.60 mol/L. (Assume T = 25°C.) Pb (b) Manu ele

Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP(1.00M) || Pb²(1.00M) | Calculate the cell potential after the reaction has operated long enough for the [Al3+] to have changed by 0.60 mol/L. (Assume T = 25°C.) Pb (b) Manu ele

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A galvanic (voltaic) cell consists of an electrode composed of manganese in a 1.01.0 M manganese(II) ion solution and a second electrode composed of lead in a 1.01.0 M lead(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 ∘C25⁢ ∘C. Use this list of standard reduction potentials.
Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP"(1.00M) | Pb³"(1.00M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al"] to have changed by 0.60 mol/L. (Assume T = 25°C.) (b) Many elements have been synthesized by bombarding relatively heavy atoms with high-energy particles in particle accelerators. Complete the fol- lowing nuclear equations, which have been used to synthesize elements. U + C-→ Cf + Cf + 'B Lr + + He Bk + in + 6 n 10 Db + 4 in 103
Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode
Consider the voltaic cell diagrammed below: Pb (s)| Pb²+ (aq)l| H2 (g)| H* (aq) | Pt (s) a) Write the balanced chemical equation that occurs in the voltaic cell depicted in the diagram. b) If the concentration of Pb2+ in this cell is 0.035 M and the pH is 1.60, what pressure of H2 (g) would keep the cell reaction in equilibrium?
For the cell: Zn(s) + 2H† (aq) →→ Zn2+(aq) + H2 (g) If [Zn2+] = 1 M, PH2 = 1 atm, and E = 0.123 V what is pH?
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Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
Silver metal can be dissolved in acidic solutions via a redox reaction with generation of hydrogen gas. Which of the following is the correct cell notation for the reaction that will occur?
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s) From the table of standard reduction potentials: Cu²+/Cu 0.337 V, E₁₂/1 Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:I AGO for this reaction would be than zero. = = 0.535 V
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Consider the voltaic cell with a standard cell potential of 0.150 V. What is the cell potential of the voltaic cell at 400 K? Cd(s) | Cd²+ (0.100 M) || Ni²+ (1.00 x 10-4 M) | Ni(s) R 8.314 J/mol-K; F = 96,485 J/mol-V O 0.239 V 0.061 V O 0.269 V O 0.031 V