Question

Use standard reduction potentials to calculate the equilibrium constant for the reaction: [ egin{array}{l} mathrm{Co}^{2+}(a q)+2 mathrm{Cr}^{2+}(a q) ightarrow mathrm{Co}(s)+2 mathrm{Cr}^{3+}(a q) \ egin{array}{|l|l|} hline mathrm{Co}^{2+}(a q)+2 e^{-} ightarrow mathrm{Co}(s) & E_{ ext {red }}^{o}=-0.280 mathrm{~V} \ hline mathrm{Cr}^{3+}(a q)+e^{-} ightarrow mathrm{Cr}^{2+}(a q) & E_{ ext {red }}^{o}=-0.410 mathrm{~V} \ hline end{array} end{array} ] Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at ( 298 mathrm{~K} ) : ( Delta G^{circ} ) for this reaction would be than zero.

          Use standard reduction potentials to calculate the equilibrium constant for the reaction:
[
egin{array}{l}
mathrm{Co}^{2+}(a q)+2 mathrm{Cr}^{2+}(a q) 
ightarrow mathrm{Co}(s)+2 mathrm{Cr}^{3+}(a q) \
egin{array}{|l|l|}
hline mathrm{Co}^{2+}(a q)+2 e^{-} 
ightarrow mathrm{Co}(s) & E_{	ext {red }}^{o}=-0.280 mathrm{~V} \
hline mathrm{Cr}^{3+}(a q)+e^{-} 
ightarrow mathrm{Cr}^{2+}(a q) & E_{	ext {red }}^{o}=-0.410 mathrm{~V} \
hline
end{array}
end{array}
]
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.
Equilibrium constant at ( 298 mathrm{~K} ) :
( Delta G^{circ} ) for this reaction would be than zero.

Use standard reduction potentials to calculate the equilibrium constant for the reaction:
[
eginarrayl
mathrmCo^2+(a q)+2 mathrmCr^2+(a q)
ightarrow mathrmCo(s)+2 mathrmCr^3+(a q) eginarray|l|l|
hline mathrmCo^2+(a q)+2 e^-
ightarrow mathrmCo(s) E ext red ^o=-0.280 mathrm V hline mathrmCr^3+(a q)+e^-
ightarrow mathrmCr^2+(a q) E ext red ^o=-0.410 mathrm V hline
endarray
endarray
]
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.
Equilibrium constant at ( 298 mathrm K ) :
( Delta G^circ ) for this reaction would be than zero.

Added by Dee W.

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