Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + 21 (aq) → Cu(s) + I2 (s) Cu²+/Cu = 0.337 V, E₂/1 = 0.535 V 12/1 From the table of standard reduction potentials: E Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:1 AGO for this reaction would be than zero.

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Use standard reduction potentials to calculate the equilibrium constant for the reaction:
2+
Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s)
From the table of standard reduction potentials: Cu²+/Cu
0.337 V, E₁₂/1
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.
Equilibrium constant at 298 K:I
AGO for this reaction would be
than zero.
=
= 0.535 V
Transcribed Image Text:Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s) From the table of standard reduction potentials: Cu²+/Cu 0.337 V, E₁₂/1 Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:I AGO for this reaction would be than zero. = = 0.535 V
Consider the following cell reaction:
Ni(s) + 2 H+(? M) ⇒Ni²+(1.00 M) + H₂(g)(1.00 atm)
If the cell potential at 298 K is 0.100 volts, what is the pH of the hydrogen electrode?
pH =
Transcribed Image Text:Consider the following cell reaction: Ni(s) + 2 H+(? M) ⇒Ni²+(1.00 M) + H₂(g)(1.00 atm) If the cell potential at 298 K is 0.100 volts, what is the pH of the hydrogen electrode? pH =
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