2+2 Fe+ (aq) + 3 Sn(s) → 2 Fe(s)+3 Sn²† (aq)Express your answer using two significant figures.ΑΣΦ?K = Calculate the equilibrium constant for each of thereactions at 25°C.Standard Electrode Potentials at 25 °CReduction Half-ReactionE° (V)Fe+(aq) + 3 e → Fe(s)-0.036Sn²+ (aq) + 2 e → Sn(s)-0.142+Cu" (ag) + 2 е — Cu(s)0.16O2 (g) + 2 H2O(1) +4 e¯ →4 OH (aq)0.40Cl2(9) + 2 е —2 CI1.36I2(s) + 2 e → 2 10.54

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2+ 2 Fe+ (aq) + 3 Sn(s) → 2 Fe(s)+3 Sn²† (aq) Express your answer using two significant figures. ΑΣΦ ? K =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.98QE

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

2+
2 Fe+ (aq) + 3 Sn(s) → 2 Fe(s)+3 Sn²† (aq)
Express your answer using two significant figures.
ΑΣΦ
?
K =

Calculate the equilibrium constant for each of the
reactions at 25°C.
Standard Electrode Potentials at 25 °C
Reduction Half-Reaction
E° (V)
Fe+(aq) + 3 e → Fe(s)
-0.036
Sn²+ (aq) + 2 e → Sn(s)
-0.14
2+
Cu" (ag) + 2 е — Cu(s)
0.16
O2 (g) + 2 H2O(1) +4 e¯ →4 OH (aq)
0.40
Cl2(9) + 2 е —2 CI
1.36
I2(s) + 2 e → 2 1
0.54

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