Given the half-cell reactions below (a) write a complete reaction: NAD* + H* + 2e NADH2 E = -0.32 V O2 + 2H* + 2e H2O2 E = +0.30 V (b) What is the AEo of the reaction? (c) What is the AG' of the overall reaction?

Given the half-cell reactions below (a) write a complete reaction: NAD* + H* + 2e NADH2 E = -0.32 V O2 + 2H* + 2e H2O2 E = +0.30 V (b) What is the AEo of the reaction? (c) What is the AG' of the overall reaction?

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

Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq) (a) (b) (c) O Strength of oxidizing agent cell V not spontaneous spontaneous Selected Standard Electrode Potentials (298 K) Half-Reaction F2(g) + 2e7 Cl₂(g) + 2e7 MnO₂(s) + 4H+ (aq) + 2e7 NO3(aq) + 4H+ (aq) + 3e¯ Ag+ (aq) + e Fe³+ (aq) + e O₂(g) + 2H₂O() + 4e Cu²+ (aq) + 2e7 2H+ (aq) + 2e7 N₂(g) + 5H+ (aq) + 4e¯ Fe2+ (aq) + 2e7 2+ Zn²+ (aq) + 2e 2H₂O() +2e7 Na+ (aq) + e 2F (aq) 2C1 (aq) 2+ Mn²+ (aq) + 2H₂O(l) NO(g) + 2H₂O(l) Ag(s) Fe²+ (aq) 4OH(aq) Cu(s) H₂(g) N₂Hs+ (aq) Fe(s) Zn(s) H₂(g) + 2OH(aq) Na(s) Strength of reducing agent E half-cell (V) +2.87 +1.36 +1.23 +0.96 +0.80 +0.77 +0.40 +0.34 0.00 -0.23 -0.44 -0.76 -0.83 -2.71
Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is given below. 2 H₂(g) + O₂(g) – 2 H₂O(l) K = 1.34×1083 (a) Calculate 8º and AG° at 298 K for the fuel-cell reaction. V Cº AGº (b) Predict the signs of AH° and ASº for the fuel-cell reaction. AH°: O O O O AS°: positive negative positive negative (c) As temperature increases, does the maximum amount of work obtained from the fuel-cell reaction increase, decrease, or remain the same? Explain. as T increases. Since AS is ---Select--- ŷ as T increases, AG becomes more ---Select--- ŷ Therefore, the maximum work obtained will ---Select--- Need Help? Read It Supporting Materials Periodic Table I Constants & Factors Supplemental Data
A voltaic cell using Cu/Cu²+ and Sn/Sn²+ half-cells is set up at standard conditions, and each compartment has a volume of 345 mL. The cell delivers 0.17 A for 31.5 h. (a) How many grams of Cu(s) are deposited? 9.7 (b) What is the [Cu²+ ] remaining? 0.56
Given the following data, answer the following questions: Fe2+(aq) + 2e- → Fe(s) E○red = -0.44 v, Cr3+(aq) + e- → Cr2+(aq) E○red = -0.407 v (a) What is the spontaneous cell reaction when a voltaic cell is constructed using these two half- reactions? (b) What is the E○ for the reaction?(c) What is equilibrium constant and deltaG?(d) If the concentration of Cr3+ and Cr2+ are each 0.10 M and the cell potential is 0.100 v, what is the concentration of Fe2+?(e) What is E for the reaction at equilibrium?
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
Pls help ASAP.
(a) In the electrolysis of aqueous Na2C204, how many liters of H2(g) (at STP) are generated by a current of 82.6 A for a period of 54.0 min? The unbalanced chemical reaction representing this electrolysis is shown below. Na2C204(aq) + H20(1) → CO2(g) + H2(g) + NaOH(aq) liters of H2(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.
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
A galvanic cell using Cu"/Cu and Cu?+/Cu was set up at 293 K and the non-standard cell potential was determined to be 0.175 V. Determine the concentration of ions in the cathode's solution if the concentration at the anode is 0.7787 M: (cathode)(M) number (rtol=0.03, atol=1e-08)
The potential, AE°, for an electrochemical cell for the reaction shown below is 0.339 V: Cu2*(aq) + H2(g) = Cu(s) + 2H*(aq) (1) What is AE° for reaction 2? ½Cu2*(aq) + ½H2(g) = ½Cu(s) + H*(aq) (2) Select your response from the list below. i) 0.339 V ii) 0.678 V iii) 0.1695 V
Including the state of reaction (aq),(l),(g),etc Thank you