4. What is the equilibrium constant of this reaction at 25 °C? 5. After 56.0 hours at 1.04 A, how many moles of electrons have been used in this reaction? 6. Predict the sign of the entropy (ASrxn) for this electrochemical reaction. Explain your reasoning.
4. What is the equilibrium constant of this reaction at 25 °C? 5. After 56.0 hours at 1.04 A, how many moles of electrons have been used in this reaction? 6. Predict the sign of the entropy (ASrxn) for this electrochemical reaction. Explain your reasoning.
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter5: Gases, Liquids, And Solids
Section: Chapter Questions
Problem 5.39P: 5-39 An 8.00-g sample of a gas occupies 22.4 L at 2.00 atm and 273 K. What is the molar mass of the...
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I need help with questions 4-6?
Transcribed Image Text:1. Find the overall reaction that will be occurring between the H₂B03/ B and
Bio+ / Bi half cells in acidic conditions.
2. What is the standard cell voltage of this electrochemical cell?
3. What is the standard free energy of this reaction?
4. What is the equilibrium constant of this reaction at 25 °C?
5. After 56.0 hours at 1.04 A, how many moles of electrons have been used in this
reaction?
6. Predict the sign of the entropy (ASrxn) for this electrochemical reaction. Explain your
reasoning.
Transcribed Image Text:x
kb = 1.38 × 10-23/
K
1 mL = 1 cm³
C
mol
1 atm = 760 torr
F = 9.648 x 104
Reaction
H₂B03 (aq) / B (s)
Bi0+ (aq) / Bi (s)
R = 8.3145
Ered (V)
-0.8698
0.320
J
mol. K
A
14=1²
1V=1/2
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