The reduction potential of ferricyanide to ferrocyanide ion occurs at +0.36 V when both ions are 1M in concentration at 25 °C. The same process occurs at +0.72 V when the medium is made 1M in HCIO4. What is the oxidation potential of ferrocyanide/ferricyanide? Eox = -0.72 V and Eoxº = -0.36 V Eox = -0.36 V and Eoxº = -0.72 V Eox = +0.36 V and Ex = +0.72 V Eox = +0.72 V and Eoxº¹ = +0.36 V

The reduction potential of ferricyanide to ferrocyanide ion occurs at +0.36 V when both ions are 1M in concentration at 25 °C. The same process occurs at +0.72 V when the medium is made 1M in HCIO4. What is the oxidation potential of ferrocyanide/ferricyanide? Eox = -0.72 V and Eoxº = -0.36 V Eox = -0.36 V and Eoxº = -0.72 V Eox = +0.36 V and Ex = +0.72 V Eox = +0.72 V and Eoxº¹ = +0.36 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The following standard reduction potentials have been determined for the aqueous chemistry of…

Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

Q: Given the following standard reduction potentials: Fe³+ (aq) + e Fe²+(aq), E°= +0.77V - O₂(g)+ 4 H…

A: The electrode which is having a higher reduction potential gets reduced at the cathode while the…

Q: Calculate the pK for the oxidation of X by Hplus at 25 degrees C. X(s) + 2 Hplus → X2 plus (aq)+…

A: Given reaction: X(s) + 2H+ ----> X2+ (aq) + 22H2 (g) half reaction: X ----> X2+ + 2e- E…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: Consider the following half reaction NO3(aq) + 10 H+ (aq) + 8e -> NH4+ (aq) + 3H₂O(1) If the ratio…

Q: Calculate the gibbs free energy (ΔGo) in kilojoules (KJ) for ColCo2+ II Cd2+I Cd The faraday…

A: In an electrochemical cell, the electrode with higher electrode potential acts as cathode. The…

Q: An electrochemical cell is constructed such that on one side a pure cadmium electrode is in contact…

Q: When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M,…

Q: A certain half-reaction has a standard reduction potential Ered=-1.18 V. An engineer proposes using…

A: The standard reduction potential at the cathode = -1.18 V The standard cell potential must be…

Q: Discuss the spontaneity of an electrolytical reaction in terms of its standard emf (Eocell)If a…

A: Spontaneous reaction can be defined as the reaction that occur by itself without any external source…

Q: The cell potential between two beakers containing copper(II) sulfate solutions and copper metal…

A: To calculate the percent error of the voltage measurement compared to the theoretical predictions,…

Q: 1. Given the electrochemical reaction shown, what is the standard free energy of change if E* =…

A: The electrical work done in a galvanic cell is the product of the electricity (charge = nF) passed…

Q: Use standard reduction potentials to determine the approximate magnitude of the equilibrium constant…

A: Given that, a redox reaction is 2Cr3+(aq) + 3Cd(s) → 3Cd2+(aq) + 2Cr(s). The redox potentials of the…

Q: %3D Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.884…

A: In an electrochemical cell, there are two compartments, the one in which oxidation reaction takes…

Q: Calculate AGexn and K for each of the following reactions. Part C The disproportionation of MnO2 (s)…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + With(so much) =…

Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 9.08x10-3 M and [Ni2+] =…

Q: The redox potentials for the Zn2+/Zn and Cl2/Cl– couples are -0.764 V and 1.395 V, respectively.…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: F = 96500 J/molVE0(I2) = 0.535 VE0) = -0.740 V

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

Q: 1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

Q: The free energy change for the following reaction at 25 °C, when [Fe²+] = 1.18 M and [Cr³+] =…

A: an electrochemical cell reaction is an example of redox process

Question

The reduction potential of ferricyanide to
ferrocyanide ion occurs at +0.36 V when both ions are
1M in concentration at 25 °C. The same process
occurs at +0.72 V when the medium is made 1M in
HCIO4. What is the oxidation potential of
ferrocyanide/ferricyanide?
Eox = -0.72 V and Exº¹ = -0.36 V
Eox = -0.36 V and Eoxº = -0.72 V
Eox
= +0.36 V and Ex = +0.72 V
Eox
= +0.72 V and Eoxº'
= +0.36 V

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A Cu electrode is immersed in a solution that is 1.00 M in [Cu(NH3)4]2+ and 1.00 M in NH3. When the cathode is a standard hydrogen electrode, the emf of the cell is found to be +0.08 V. What is the formation constant for[Cu(NH3)4]2+?
Calculate the EMF of the following electrochemical cell: Pt | VO2+(0.25 M), V3+(0.10 M), H+ (0.001 M) || TI3+ (0.10 M), TI+(0.05 M), | Pt Indicate whether the cell is galvanic or electrolytic. Evo2+/v3+ = 0.361 V, ET³+/T+ = 1.25 V Ans: 1.23 V, galvanic
The free energy change for the following reaction at 25 °C, when [Cd2*] = 1.17 M and [Cr+] = 8.47x10-3 M, is -207 kJ: 3ca**(1.17 M) + 2Cr(s)3Cd(s) + 2Cr³+(8.47x103 M) AG = -207 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
K124.
A fluoride ISE immersed in 1 x 10•2 mol dm solution of sodium fluoride gives a potential of 35,2 mV and when it is immersed in a tooth paste solution it gives a potential of 30,2 mV. What is the concentration of fluoride ion in the toothpaste?
The F− concentration of a solution was determined by measurements with a liquidmembrane electrode. The electrode system developed a potential of 0.5021 V when immersed in 25.00 mL of the sample, and 0.4213 V after the addition of 2.00 mL of 5.45 x 10−2 M NaF. Calculate pF for the sample.
Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an important biological reaction.Below are the reduction reactions and standard reduction potentials (E °) at pH = 7 and 25 ° C.Pyruvate + 2H + + 2e- = Lactate - (E ° = -0.185 V)Cytochrome C (Fe3 +) + e - = Cytochrome C (Fe2 +) (E ° = 0.254 V) Considering the Gibss free energy and Nernst equations, calculate the following equilibrium ratio (K) at 25 ° C, pH = 7.
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.