The electrode which act as anode the potential of the voltaic cell has to be determined. Concept introduction: According to the first law of thermodynamics , the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system. The equation is as follows. ΔU = Q - W ΔU = Change in internal energy Q = Heat added to the system W=Work done by the system In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell. ΔG 0 = -nFE 0 n = Number of moles transferred per mole of reactant and products F = Faradayconstant=96485C/mol E 0 = Volts = Work(J)/Charge(C) The relation between standard cell potential and equilibrium constant is as follows. lnK = nE 0 0 .0257 at 298K The relation between solubility product K sp and equilibrium constant is as follows. K sp = e +lnK
The electrode which act as anode the potential of the voltaic cell has to be determined. Concept introduction: According to the first law of thermodynamics , the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system. The equation is as follows. ΔU = Q - W ΔU = Change in internal energy Q = Heat added to the system W=Work done by the system In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell. ΔG 0 = -nFE 0 n = Number of moles transferred per mole of reactant and products F = Faradayconstant=96485C/mol E 0 = Volts = Work(J)/Charge(C) The relation between standard cell potential and equilibrium constant is as follows. lnK = nE 0 0 .0257 at 298K The relation between solubility product K sp and equilibrium constant is as follows. K sp = e +lnK
Solution Summary: The author explains that the potential of the voltaic cell is directly related to the free energy difference between the reactants and products in the cell.
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
Chapter 19, Problem 83GQ
Interpretation Introduction
Interpretation:
The electrode which act as anode the potential of the voltaic cell has to be determined.
Concept introduction:
According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system.
The equation is as follows.
ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system
In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.
ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol E0= Volts = Work(J)/Charge(C)
The relation between standard cell potential and equilibrium constant is as follows.
lnK = nE00.0257 at 298K
The relation between solubility product Ksp and equilibrium constant is as follows.
Complete the following acid-base reactions and predict the direction of equilibrium
for each. Justify your prediction by citing pK values for the acid and conjugate acid in
each equilibrium.
(a)
(b) NHs
(c)
O₂N
NH
NH
OH
H₁PO₁
23.34 Show how to convert each starting material into isobutylamine in good yield.
ཅ ནད ཀྱི
(b)
Br
OEt
(c)
(d)
(e)
(f)
H
Please help me Please use https://app.molview.com/ to draw this. I tried, but I couldn't figure out how to do it.
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