Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction:...
Part C Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction Zn(s) +Fe2(a)Zn2+ Fe(s) Report the answer in volts with three significant figures. LA Value Units Request Answer Submit Part D Determine the equilibrium constant for the above reaction Report to 1 significant figure and using scientific notation. ΑΣ Submit Request Answer
Part A Write a chemical equation for the reaction that occurs in the following cell: CuCu?+ (aq)||Ag+ (aq)|Ag. Cu(s) + 2Ag+ (aq) +Cu2+ (aq) + 2Ag(s) Previous Answers Correct Part B Given the following E's, calculate the standard-cell potential for the cell in the question above. Cu²+ (aq) + 2e +Cu(s) E° = +0.50 V Ag (Aq) + +Ag(8) E° = +0.76 V A2¢ * OO? Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
question 1 - Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe3+(aq) + Cu+(aq) Fe2+(aq) + Cu2+(aq) Carry at least 5 significant figures during intermediate calculations to avoid roundoff error when taking the antilogarithm. Equilibrium constant: ..... ? G° for this reaction would be greater or less than zero.? question 2 Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2+(aq) + Hg(l)2Cu+(aq) + Hg2+(aq) Carry at least 5 significant figures during intermediate...
Use the References to access in Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2 Ag+ (aq) + Fe(s) —2Ag(s) – Fe2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant AGº for this reaction would be than zero Submit Answer Try Another Version 2 item attempts remaining
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu2 (aq)Fe2 (aq)>Cu (aq) + Fe3 (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant than zero AGo for this reaction would be Submit Answer Retry Entire Group 9 more group attempts remaining Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd2(aq)21(aq)>Cd(s)I2(s) Hint: Carry at least 5 significant figures during intermediate...
Use the following standard cell potentials to answer the questions below. Fe3+(aq) + e− ⇌ Fe2+(aq) E° = 0.771 V Ag3+(aq) + e− ⇌ Ag2+(aq) E° = 1.800 V 1. What is ΔG° (in kJ/mol) for this reaction? Report answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol) 2. This reaction is (spontaneous/not spontaneous)
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu2+(aq) + 2Fe2+ (aq) +Cu(s) + 2Fe+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant AGⓇ for this reaction would be than zero.
Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V