Find the equilibrium constant for a 3-electron transfer process, whose standard emf is #"0.59 V"# at #"298.15 K"#? #F = "96485.33 C/mol e"^(-)#
#a)# #10^15#
#b)# #10^20#
#c)# #10^25#
#d)# #10^30#
where
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The equilibrium constant (K) for a 3-electron transfer process with a standard electromotive force (emf) of 0.59 V at 298.15 K and Faraday's constant (F) of 96485.33 C/mol e^(-) can be calculated using the Nernst equation:
K = exp((-n*E°) / (RT))
Where:
- n is the number of electrons transferred (3 in this case)
- E° is the standard emf (0.59 V)
- R is the gas constant (8.314 J/(mol*K))
- T is the temperature in Kelvin (298.15 K)
Substituting the values:
K = exp((-3 * 0.59) / (8.314 * 298.15))
K ≈ exp(-1.7746 / 2477.883)
K ≈ exp(-0.000715)
K ≈ 0.9993
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