A galvanic cell is made of a Ni2+/Ni half cell with [Ni²*] = 6.00 × 10-² M and an Ag*/Ag hal cell with [Ag*] = 4.00 × 10-3 M. Calculate the electromotive force of the cell at 25 °C. The reduction potentials for the two half reactions: E° = -0.24 E° = +0.8 Ni2* (aq) + 2e¯ →Ni(s) Ag*(aq) + e¯ →Ag(s) О а. 1.06 O b. 1.04 О с. 0.94 O d. 0.64 О е. 1.14

A galvanic cell is made of a Ni2+/Ni half cell with [Ni²] = 6.00 × 10-² M and an Ag/Ag hal cell with [Ag] = 4.00 × 10-3 M. Calculate the electromotive force of the cell at 25 °C. The reduction potentials for the two half reactions: E° = -0.24 E° = +0.8 Ni2 (aq) + 2e¯ →Ni(s) Ag*(aq) + e¯ →Ag(s) О а. 1.06 O b. 1.04 О с. 0.94 O d. 0.64 О е. 1.14

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

A galvanic cell is constructed using the following half-reactions at 298 K. Given Kf = 1.0 x 10^8 for MX4^2+ calculate the cell potential.MX42+(aq) + 2e– ⇌ M(s) + 4X(aq) [MX42+] = 0.100 M and [X] = 4.00 MM2+(aq) + 2e– ⇌ M(s) [M2+] = 0.100 M
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AGren-79 kJ/mol. If the concentration of Fe2 is increased to 2.0 M, then Ecell will and AGren will be. Fe(s) + 2H(aq) →→→→ Fe²+ H₂(g) O increase, less negative O decrease, more negative decrebe, less negative O increase, more negative than AG
Calculate the cell potential given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.57 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.41 V
Using the following standard reduction potentials, 34 Fe *(aq) + e - Fe2*(aq) Ni2*(ag) + 2 e -Ni(s) E° = +0.77 V E° = -0.26 V calculate the standard cell potential for the cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions 34, Ni 2*( aq) + 2 Fe 2*( aq) → 2 Fe *( aq) + Ni( s) E° = +1.03, nonspontaneous E° = + 1.03, spontaneous E° = -1.03 V, spontaneous E° = -1.03 V, nonspontaneous
13) The average C−C bond dissociation energy (D) is 350 kJ/mol and the average C=C bond dissociation energy is 728 kJ/mol. Based on these values, which is stronger: a σ or a π bond?
Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– → Pt(s); E° = 1.18 V Cr2O72–(aq) + 14 H+(aq) + 6 e– → 2 Cr3+(aq) + 7 H2O(); E° = 1.33 V Which of the following is the strongest oxidizing agent? Fe Pt Cr^3+ Fe^2+ Cr2O7^2-
A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00 x 10–4 M in the two half-cells. The reduction potential of Ni2+ is –0.23 V. Calculate the potential of the cell at 25°C.
Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, E for the reaction. E = V cell Calculate the equilibrium constant, K, for the reaction. K =
Calculate the cell potential, E, for the given reactions at 25.00 "C using the ion concentrations provided. Then, determine if th cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E). Pt(s) + Fe²(aq) = P² (aq) + Fe(s) [Fe²*1 = 0.0064 M E= incorrect -4761 E= Cu(s) + 2 Ag* (aq) = Cu² (aq) + 2 Ag(s) |Cu²+1 = 0.027 M Ag1=0.027 M E [P1²*1 = 0.067 M Co² (aq) + Ti (aq) — Co¹ (aq) + Ti² '(aq) Co²1 = 0.055 M Co= 0.030 M ITP 1 = 0.0070 M T² = 0.0107 M mam V The cell is not spontaneous spontaneous. The cell is spontaneous not spontaneous. incorrect The cell is spontaneous not spontaneoux.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGO for the following redox reaction. Be sure your answer has the correct number of significant digits. 2 MnO₂ (s) + 80H(aq) + 3Cl₂ (g) → 2 MnO4 (aq) + 4H₂O(1) +6Cl¯¯ (aq) 2 kJ x10 X S ? olo Ar
Given the following2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq) E°cell = 0.73 V and AgCl(s) → Ag(s) + Cl-(aq) E°= 0.222 V What is the standard reduction potential for X2+(aq)?
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: (aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq) AG° Pb²+ = Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V red 2+ Cu²+ (aq) + e → Cu+ (aq) Fº red kJ K for this reaction would be = = 0.153 V + than one.