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In the mitochondria of human cells, energy is provided by the oxidation and reduction of the iron ions in the cytochromes. Identify each of the following reactions as an oxidation or reduction:
a.
b.
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- (7.12) A technician plates a faucet with 0.86 g Cr metal by electrolysis of aqueous Cr2(SO4)3. If 12.5 min is allowed for the plating, what current is needed? Molar mass of Cr: 51.996 g/mol Analysis/Strategy: mass of Cr ® mol Cr mol e¯ (or Faraday) ® coulombs ® amperes Reduction half-reaction of chromium solution to chromium metal: Cr* ,+3, (aq) e¯ ® Cr(s) + chromium solution, Cr2(SO4)3, has the ions: [Cr*3 s04-²] Answer: The current needed is ampere. (2 sig fig)arrow_forwardFill in the blanks: (7.14) In the electrolysis of CUSO4, how much copper is plated out on the cathode by a current of a 0.75A in 10 minutes? (Cu 63.546 g/mol) Analysis/Strategy: ampere & time coulombs ® mol e¯ (or Faraday) ® mol Cu (R mass of Cu Reduction half-reaction of copper solution to copper metal: Cu*²(aq) + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2 SOq] Answer: The mass of copper plated out is g Cu. (3 sig fig)arrow_forward(7.9) Using potentials listed in the Table, the standard reduction determine whether the following reaction is spontaneous under standard conditions. Support your answer. Hg*2(aq) + 21¯(aq) → ,+2, Hga) +I2(s) From the Table: Hg*2(aq) + 2e¯ → Hga) E°red = +0.85 V I2(s) + 2e- - 21 (aq) E°red = +0.54 V Answer: Is the above reaction spontaneous? (YES or NO) Briefly support your answer (. Refer to the Table of Standard Reduction Potential below. STANDARD REDUCTION POTENTIAL AT 25 °C ETV) atteaction +0.50 2H,O + 2e-Hlg) + 20H (a Hait-Reaction (V) Ag (ag) +- Agis) Aglle(s)+- Ag)+ r (a) AgCIs) - Ag(s) -a(ap) Ag(CN), (a) eAgs)+ 2CN (a) -O83 Agi+ r(a) 0.10 HO, (a) + HO) + 2e 3OH (a) +0.22 HOa) + 2H(ag) 2e 2Ho) -0.31 He(a 2e 2 Hg) +0.45 2Hg"(a)+ 2e Hg () -0.15 He(a)+ 2e Hel) ) + 2e 21(a) -1.46 2 10, (a) + 12H(a) + 10e l) +6HO) +0.56K'(ag) K) +1.78 a79 AgCro,(s) + 2e 2 Ags) + Cro ) Agl(s) +e- Ag) (a) AgrS,0(a) + - Agis) + 25,0 (a) A" (a) + 3e - A) 92 054 1.20 HAs0,n- 2H"(a) + 2e HAOa) + H,o)…arrow_forward
- Complete and balance the following redox reaction in basic solution Zn(s) → Zn(OH),*(aq) + H,(g) 4 4- 2- D2+ 3+ 4+ + 1 2 3 4 6. 7 8 9. O3 O6 O7 (s) (1) (g) (aq) + e Zn H* OH Reset • x H,0 Delete 9. 4. 3. 2.arrow_forward(7.4) Describe in shorthand notation a galvanic cell for which the cell has the following reaction. Chose the BEST option by writing the CAPITAL LETTER of the best answer. Cu(s) + 2 Fe*3(aq) - Cu*?(aq) + 2 (be). Fe2 (aq) CHOICES: (A) Cu Cu*2||Fe*3|Fe*2 (B) Cu*2|Cu||Fe*3| Fe*2 (C) Cu|Cu*2||Fe*2 |Fe*3 (C) Cu*2|Cu||Fe*2| Fe*3 Answer:arrow_forwardFill in the blanks: (7.13) Using a current of 4.75 A, how many minutes does it take to plate a sculpture with 1.50 g of Cu from a CuS04 solution? (Cu 63.546 g/mol) Analysis/Strategy: mass of Cu ® mol Cu ® mol e" (or Faraday) ® coulombs ® time in minutes (given current in amperes) Reduction half-reaction of copper solution to copper metal: Cu*2(aq) · + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2_SOq] Answer: The time needed to plate out a sculpture is minutes. (3 sig fig)arrow_forward
- (7.15a) What mass of copper is plated out in the electrolysis of CUSO4, in the same time that it takes to deposit 1.00g of Ag in a silver coulometer that is arranged in series with CUSO4 cell? (7.15b) If a current of 1.00 A is used, how many minutes is required to plate out this quantity of copper? Molar Mass (g/mol): Cu 63.546 Ag 107.87 Analysis/Strategy: ampere & time coulombs ® mol e¯ (or Faraday) ® mol ® Cu ® mass of Cu time to plate out Cu = time to plate out 1.00 g Ag (in series with CuSO4 cell) Reduction half-reaction of silver metal: Ag*(aq) + e ® Ag(s) Reduction half-reaction of copper metal: Cu*2(aq) + e ® Cu(s) Answer: Mass of copper plated out = g (3 sig fig) Minutes required to plate out copper using 1.00 ampere = minutes (3 sig fig)arrow_forward(7.15a) What mass of copper is plated out in the electrolysis of CuSO4, in the same time that it takes to deposit 1.00g of Ag in a silver coulometer that is arranged in series with CUSO4 cell? (7.15b) If a current of 1.00 A is used, how many minutes is required to plate out this quantity of copper? Molar Mass (g/mol): Cu 63.546 Ag 107.87 Analysis/Strategy: ampere & time coulombs ® mol e¨ (or Faraday) ® mol Cu mass of Cu time to plate out Cu = time to plate out 1.00 g Ag (in series with CUSO4 cell) Reduction half-reaction of silver metal: Ag"(aq) + e ® Ag(s) Reduction half-reaction of copper metal: Cu*²(aq) 1+2, + Cu(s)arrow_forward(7.8) A voltaic cell is based on Co*2/Co half- cell and a AgCl/Ag half-cell. a) What reaction occurs at the anode? b) What is the standard cell potential, E°cell ? (a) Choices: The reaction that occurs at the anode: (A) Co*2(aq) + 2e¯ ® Co(s) (B) Co(s) ® Co²(aq) +2, + 2e- (C) Ag*(aq) + e¯ ® Ag(s) (D) Ag(s) ® Ag* (aq) + e¯ Answer: The reaction that occurs at the anode is (CAPITAL LETTER only). b) What is the standard cell potential, E°cell ? Choices: (A) +0.52 V (C) -0.52 V (B) -1.08 V (D) +1.08 V Answer: The standard cell potential of the cell, E°cell = V. Refer to the Table of Standard Reduction Potential below. STANDARD REDUCTION POTENTIAL AT 25 °C Retie Hall eaction Ag'ay+e Agls) Agle) Ag) + r"(ag) AgCs) +- Ag) 0.0 2 H0)+ 2e Hl)+ 20H Tng 0.10 HO, (a) + HAXn + 2e 3OH(a) +0.22 HO) + 2H() + 2e-2H0 -0. Hea 2 2 Ha 0.45ag (a) + te He"( AgCN, (a+ r- Ag) + 2CN (a) Ag:CrO) 2e 2Ag) Co/ Aglis - Ag +F) +0.79 AgSOl - Ag) + 25,0 (ag) A la+ 3e - AA als) + 2e 2(a) +1.20 Ha ag + 2() + 2- HO + H,0)…arrow_forward
- (7.3) Write the half-cell reactions for each of the following cells. Choose from the given options the BEST answer. Write the CAPITAL LETTER of your cholce. (a) Ag I Ag* a H* I Hz 1 Pt Answer: Half-cell reactions: (A) ) & () (B) ) & (iv) (C) (i) & () (D) (i) & (iv) O Agʻ(aq) o Agts) + e Ci) Agts) Ag'laq) + Clii) 2 H"(aq, IM) 2e" - Hzg 1 atm) (iv) Hag 1 atm) - 2 H'taq, IM) * 2e I Brzn PE Answer: Hall-cell reactions: (w W& Cii) (B) (im & (i) (C) (1) & (iv) & (iv) (D) (i) Crz0, ng • 14 H'cag) *• 6e Ge 2 Cr*tag) + 7 H,0D (ii) 2 Br 2e O Brzn (iv) Brzo 2 Br+ 2earrow_forward(27) What is the value of the equilibrium constant (Keq) when the following redox reaction takes place at 727°C? Mn (s) + Sn¹+ (aq) → Mn²+ (aq) + Sn²+ (aq) (A) 2.55 x 10¹3 (B) 2.76 x 10¹8 (C) 7.62 x 1036 (D) 5.23 x 10-15 (E) 3.62 x 10-1⁹ The most convenient form of the equation for this one might not be on your note sheet. I suggest using: RT ECELL -In K nF (28) An archaeologist claims that a bone in her collection is from a saber-toothed tiger that is believed to have the carbon-1arrow_forward(7.11) A voltaic cell is constructed that uses the following reaction and operates at 298 K: Zn(s) + Cd+2, Cd*2(aq) ® + (S)uZ Zn*2(aq) + Cd(s) a) What is the emf of the cell under standard conditions? Zn*2 (ag) + 2e¯ ® Zn(s) E°cell = -0.76 V cd*2 (aq) + 2e¯ ® Cd(s) E°cell = -0.40 V Answer: The emf of the cell is V. Refer to the Table of Standard Reduction Potential below to solve Question (a). STANDARD REDUCTION POTENTIAL AT 25 °c E() Hall Reaction +0.N0 2 H,O) + ze Hg) + 2OH (a) Hal-Reaction Hall-Reaction E(V) Ag"(ng) +e- Ag(s) --0.83 Aglir(s) +e- Ag(s) + Br (ag) AgCKs) +e- Ag(s) + a"(a) Ag(CN), "(a) +e Ag(s)+ 2CN (a) Ag:Cro(s) + 2e 2 Ag(s) + Cro (ag) +0.10 HO, (a) + H,O) + 2e 3OH (ay) +0.22 H,O(ng) + 2H"(ag) + 2e 2 H;O() -0.31 Hg/ (a) + 2e 2 Hg() +0.45 2g"(ay) + 2e 1Hg (a) -0.15 Hg" (a) + 2e - Hg() +0.01 s) + 2e 21(a) +1.78 +0.79 +0.92 Agl(s) +e- Ag(s) +I(ay) +0.85 Ag(S0,) (ay) +e Ag(s) + 2 S,0 (ap) +0.54 A (ay) + 3e Al(s) HAso,(a) + 2H'(ay) + 2e - HAsOdany) + HO() Ba"(ag) + 2e -…arrow_forward
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