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 value (in V) of E°cel| for the following reaction? Pb 2+ (aq) + Be (s)→ Pb (s) + Be?+ (aq)
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)
(a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 91.2 A for a period of 60.1 min? The unbalanced chemical reaction representing this electrolysis is shown below.NaCl(aq) + H2O(l) Cl2(g) + H2(g) + NaOH(aq)__________ liters of Cl2(g) is generated by this electrolysis.(b) How many moles of NaOH(aq) are formed in the solution in this process? _______moles of NaOH(aq) are formed.
None
If you want to reduce Sn+ to Sn2* and you have Fe2*, Fe, Al (s), and Al3+ available. What chemical would you mix with Sn+? Write the overall redox reaction that will OCcur. E° (V) A13+ + 3e Al(s) -1.66 Sn+2e Sn2+ 0.14 Fe + e Fe2+ 0.77 Note: This question may be easier to submit through your handwritten work only.
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
Using the Nernst equation, determine the Ecell at 25 °C for the following reaction in 1.0M HCI: [Cu²*] = 2.5M Cu(s) + MnO4¬(aq) → MnO2(s) + Cu2*(aq) [MnO4¯] = 0.10M
urgent
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+…
None