Ch.18 - ElectrochemistrySee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Calculate the standard free energy change (kJ) for the following reaction using the standard electrode potentials. Sn(s) + Ni2+(aq)  ⇌  Sn2+(aq) + Ni(s)          Ni 2+(aq) + 2 e - → Ni(s)        E° = -0.25 V          Sn2+(aq) + 2 e - → Sn(s)        E° = -0.14 V                      A. +10                      B. -10                      C. +15                      D. -21                      E. +21

Problem

Calculate the standard free energy change (kJ) for the following reaction using the standard electrode potentials.

Sn(s) + Ni2+(aq)  ⇌  Sn2+(aq) + Ni(s)

         Ni 2+(aq) + 2 e - → Ni(s)        E° = -0.25 V

         Sn2+(aq) + 2 e - → Sn(s)        E° = -0.14 V

                     A. +10

                     B. -10

                     C. +15

                     D. -21

                     E. +21