A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides.The following reaction describes the formation of NO, oneof the products.3Cu(s) + 8H* (aq) + 2NO,(aq)→ 2NO(g) +3Cu²+(aq)+4H,0(1)E°cell for this reaction is 0.620 V.1st attemptFeedbacki See Periodic Table O See HintWhat is the value of E°,at 300 K when [H*] = 0.100 M, [NO3] = 0.0250 M, [Cu2*] = 0.0350 M, and the partial pressure of NO isrxn0.00180 atm? 8 -4.4515V

A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides.The following reaction describes the formation of NO, one of the products. 3Cu(s) + 8H*(aq) + 2NO,(aq) → 2NO(g) +3CU²+ (aq) + 4H,0(1) E° cel for this reaction is 0.620 V. 1st attempt Feedback See Periodic Table O See Hint What is the value of E° Pxn at 300 K when [H*] = 0.100 M, [NO3¯] = 0.0250 M, [Cu²*] = 0.0350 M, and the partial pressure of NO is 0.00180 atm? O -4.4515 V

A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides.The following reaction describes the formation of NO, one of the products. 3Cu(s) + 8H(aq) + 2NO,(aq) → 2NO(g) +3CU²+ (aq) + 4H,0(1) E° cel for this reaction is 0.620 V. 1st attempt Feedback See Periodic Table O See Hint What is the value of E° Pxn at 300 K when [H] = 0.100 M, [NO3¯] = 0.0250 M, [Cu²*] = 0.0350 M, and the partial pressure of NO is 0.00180 atm? O -4.4515 V

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...

See similar textbooks

Similar questions

What is the correct shorthand notation for the cell on the previous slide? Oxidation: Ag(s) Ag*(aq) + e- Reduction: Mno,(s) + 4 H*(ag) + 2 e - Mn2+(aq) + 2 H,0() A. Ag(s) | Ag*(aq) || H*(aq), Mn²*(aq), H20() | MnOg(s) В. Ag*(aq) | Ag(e) || Mn02(a) | Mn²*(aq), H20(). H*(aq) C. Mno2(3) | H*(aq), Mn²*(aq), H20() || Ag*(aq) | Ag(3) D. Mn2*(aq). H20(). H*(@q) | MnO2(s) || Ag(3) | Ag*(aq)
Determine the values of E°cell for the reaction with the following half reactions: O2(g) + 4 H+(aq) + 4 e– → 2 H2O(l) E° = +1.229 V 4 I–(aq) → 2 I2(s) + 4 e– E°= –0.535 V
None
Question 11.d of 14 Submit Consider the following equation in aqueous solution: PO,3-(aq) + SO2(g) → PO,3-(aq) + S²-(aq) Write the balanced half-reaction for the oxidation in acidic solution. PO3 (aq) + 2 e + H2O (1) → PO,* (aq) + 4 2 H'(aq)| 3C,2- Reset > 1 3 4 8 + ) -> (s) (1) (g) (aq) e H2O H* H;0* H. • x H2O P. LO
Determine E°cell for the reaction below. 3 D2 (l) + 2 Z (s) → 2 Z3+(aq) + 6 D–(aq) Z3+(aq) + 3 e– → Z (s) E° = –0.04 V D2 (l) + 2 e– → 2 D– (aq) E° = +1.36 V Group of answer choices -1.40 V +1.32 V -1.32 V +4.16 V +1.40 V
(A) -0.23 V (C) -1.23 V (B) -0.85 V (D) -1.69 V 41. What is observed if a piece of lead is placed in an aqueous solution of Cu(NO3)2? Half-Reaction Pb²+ (aq) + 2e → Pb(s) Cu²+ (aq) + 2e → Cu(s) Eº, V -0.13 +0.34 I. The mass of the metal piece increases. II. The blue color of the solution becomes less intense. (A) I only (B) II only (C) Both I and II (D) Neither I nor II 42. If water is electrolyzed for 2.0 hr with a current of 10.0
14.107 Consider the reaction that takes place in a lead-acid battery when it discharges: Pb (s) + PbO₂ (s) + 2H₂SO4 (aq) → 2PbSO4 (aq) + 2H₂O (1) Which of the following statements regarding the discharge of this battery is correct? Choose the best answer. A The oxidizing agent is Pb(s). B Pb(s) is reduced. C PbO₂ is the reducing agent. D The pH decreases as the battery discharges. E The concentration of H₂SO4 decreases as the battery discharges. O O O
3:19 PM Thu May 4 * 8 J ↑ M ● ( 9 K 8 H x H₂O O O 9 L cmd = (aq) P H3O+ "' X 0 : ; { [ 300 option ? 1 50 69% Ï Submit 1 delete 1
just a&b
What are E°cell and ΔG° of a redox reaction at 25°C for which n=2 and K=0.065?
| Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- -Cr(s) Fe2+ (aq) -0.74 + 2e- -Fe (s) -0.440 Fe3+ (aq) + e- - Fe2+ (s) Snt+ (aq) +0.771 + 2e- - Sn2+ (aq) +0.154 Which of the following reactions will occur spontaneously as written? 2Cr (s) + 3FE2+ Sn4+ (ag) + Fe2+ 3FE2+ (ag) + Cr3+ (aq) → Cr (s) + 2Cr3+ (ag) + 3Sn2+ (aq) → 3Sn4+ (aq) + 2Cr (s) (s) → 3Fe (s) + 2Cr3+ (aq) (s) → Sn2+ (aq) + Fe (s) 3FE3+ (aq)
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…