Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd²+ (aq) + Hg(1)→ Cd(s) + Hg²+ (aq) From the table of standard reduction potentials: E =-0.403 V, EHg²+ /Hg = = 0.855 V Cd²+/Cd Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be than zero.

Chemistry
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Chapter1: Chemical Foundations
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Use the References to access important values if needed for this
question.
Use standard reduction potentials to calculate the
equilibrium constant for the reaction:
2+
Cd²+ (aq) + Hg(1)→ Cd(s) + Hg²+ (aq)
From the table of standard reduction potentials:
E
= -0.403 V, EHg²+ /Hg
= 0.855 V
2+
Cd²+/Cd
Hint: Carry at least 5 significant figures during intermediate
calculations to avoid round off error when taking the
antilogarithm.
Equilibrium constant at 298 K:
AGO for this reaction would be
Submit Answer
Retry Entire Group
9 more group attempts remaining
than zero.
Transcribed Image Text:Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cd²+ (aq) + Hg(1)→ Cd(s) + Hg²+ (aq) From the table of standard reduction potentials: E = -0.403 V, EHg²+ /Hg = 0.855 V 2+ Cd²+/Cd Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Submit Answer Retry Entire Group 9 more group attempts remaining than zero.
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