Answered: 3- Calculate the exact half-cell…

Science

Chemistry

3- Calculate the exact half-cell potential of Co in 0.01 M CoCl2 .

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: A student does an experiment to determine the molar solubility of lead(II) chloride. He constructs a…

Q: Suppose 30.0 mL of 0.100 M Pb(NO3)2 is added to 60.0 mL of 0.150 M KI. How many grams of Pbl2 will…

Q: The standard cell potential for the reaction: A (s) + B2* (aq) = A2* (aq) + B (s) is - 0.371 V. What…

Q: The following electrochemical cell is constructed at standard state: Mg(s) | Mg2+ || Cr2+ | Cr(s) a)…

A: Answers are explained below.

Q: Calculate AGixn and Eo (cell

Q: 10. Calculate the potential of the following cells: a) a galvanic cell consisting of a lead…

A: Given: Pb2+ =0.0848 MZn2+=0.1364 M TiO2+ =0.00146 M Ti3+ =0.02723

Q: X(s)|X3+ (2.04 M) || Mn O4 1 minus (1.62 M)|Mn2+ (0.25 M)|H+ (2.64 M) The reduction potential for…

A: Given The concentration of X3+ is 2.04 M. The concentration of MnO4- is 1.62 M. The concentration…

Q: The value of K, for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br°(aq)…

A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq) E°=0.070 V The Ksp value 5.4×10-13

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

Q: Calculate the cell potential of each of the following electrochemical cell at 25oC. b. Pt|H 2 (1.00…

A: pH = 5.97 at Anode pH = 3.47 at cathode

Q: The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2+(aq) →…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: The standard cell potential E0 for the cell reaction: Zn + Cu2+ à Zn2+ + Cu is…

A: Given :- Zn + Cu2+ → Zn2+ + Cu E°cell = 1.100 V [Zn2+] = 0.01 M [Cu2+] = 1.0 M To calculate :-…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+. Initial concentrations: [Ni2+] =…

Q: A student does an experiment to determine the molar solubility of lead() iodide. He constructs a…

A: Nernst equation gives the relation between cell potential (Ecell), standard cell potential (Ecell°),…

Q: Given an electrochemical cell containing Mg(s) and 0.10 M Mg2+ in one cell compartment and Fe(s) and…

A: All the necessary calculations have been done in the following step.

Q: 2+ 3. Given that the whole standard potential of a Zn-Mg cell is +1.61V and the standard reduction…

Q: Calculate AG° for the following cell: Pt|I (aq) | 12 (s) || Sn+ (aq), Sn²* (aq)| Pt Report your…

A: Change in standard gibbs free energy calculation for a redox reaction occurring in a electrochemical…

Q: How do I calculate the cell potential of this situation?

A: We have given a galvanic cell in which [Ti3+] = 0.02723 M [TiO2+] = 0.00146 M pH = 3 ESHE = 0.00V…

Q: The cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

A: The cell potential is calculated by Nernst equation . E = E° - (0.0591/n) log Qc E = cell potential…

Q: A standard Ag/Ag+ half cell is connected to a standard Cr/Cr3+ half cell. Calculate the standard…

A: On the basis of Reduction potential, the substances which have the lower reduction potentials are…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr*] = 0.810 M and…

A: The cell reaction given is, => Cr (s) + Fe2+ (aq) ⇔ Cr2+ (aq) + Fe (s) Given: [Cr2+ ] = 0.810 M…

Q: X(s)|X1+ (0.99 M) || Mn O4 1 minus (0.18 M)|Mn2+ (1.90 M)|H+ (2.64 M) The reduction potential for…

A: The reduction potential of X+1 = 0.32vThe reduction potential of MnO4- = 1.51v

Q: If at 25°C the standard electrode potential of the Ag/Ag* electrode is 0.799 V, and the equilibrium…

Q: Which is the best oxidizing agent in the following set? You may use the table of standard cell…

A: Oxidizing agent

Q: A student does an experiment to determine the molar solubility of lead(II) bromide. She constructs a…

Q: 3- Calculate the exact half-cell potential of Co in 0.01 M CoCl2.

A: Given, The concentration of CoCl2 = 0.01 M The half cell reaction Co→Co2+ +2e-

Q: What is the cell potential for a cell with a 2.789 M solution of Zn2+ (aq) and 0.1408 M solution of…

A: We have to find cell potential for a cell with a 2.789 M solution of Zn2+ (aq) and 0.1408 M solution…

Q: What is the Eθ cell value for a galvanic cell constructed using cadmium and copper electrodes.

A: Given:- Galvanic cell of Cd and Cu. •From electrochemical series Cd is more reactive than Cu. •Cd…

Q: A silver wire coated with AgCl is sensitive to the presence of chloride ion because of the half-cell…

A: Concentration of CuSO4 solution = 1 (M) Measured cell potential = 0.0518 V

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: Given-> E°Ni2+/Ni = -0.25 V E°Co2+/Co = -0.28 V

Q: Calculate the standard potential of this cell: Ni(s) | Ni2+(aq) || Cu2+(aq) | Cu(s). E∘=?

Q: Calculate the actual cell potential (E) at 25.0 oC for the following redox reaction when the…

A: The question is based on concepts of electrochemistry. we have been given a galvanic cell. we have…

Q: Use the standard half cell potentials listed below to calculate the standard cell potential for the…

Q: Calculate the actual cell potential if you have a 1 M solution of MgSO4, but only a 0.5 M solution…

Q: a galvanic cell is constructed of a standard half-zinc element and a chromium electrode immersed in…

A: Given information: Standard half-zinc element

Q: Calculate the standard cell potential for this reaction.

A: Here, we have to find the standard cell potential for the given reaction using the standard…

Q: For the galvanic cell 2Ag+ + Cr → 2Ag + Cr2+, which equation allows you to correctly calculate…

A: E°cell = 2.5122 V

Q: Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1…

A: Here, in the given cell notation, first of all the notation has to be understood. Pt | Cl- (1 M) |…

Q: ELECTROCHEMISTRY: Calculate the cell potential of a voltaic cell given the following standard…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.3 M NISO4 solution…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

Q: What is the Eθ cell value for a galvanic cell constructed using aluminium and nickel electrodes.

A: Foe finding Standard EMF of cell, we must know about the standard reduction potential values for the…

Q: Calculate the half-cell potential of cadmium in 0.1 M CdCl2.

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

Q: Use the tabulated electrode potentials to calculate △Grxn for the following reaction at 25 °C 2 Fe^3…

A: Gibbs free energy is state function , it does not depend on the path ∆G = ∆H-T∆S

Question

1- Calculate the theoretical tendency of Zinc to corrode with evolution of
hydrogen, when immersed in 0.001M ZNC12 acidified to pH=2.
2- The emf a cell made of Zinc (anode) and hydrogen electrode (cathode)
immersed in 0.3M ZnCl2 is +0.590V. What is the pH of the solution?
3- Calculate the exact half-cell potential of Co in 0.01 M CoCl2 .
4- Calculate the theoretical tendency of Nickel to corrode in water of
pH=7.Assume corrosion products are H2 and Ni(OH)2 the solubility
product of which is 1.8x10-15.
5- A solution is made up to contain 0.01 M NaOH. What is the theoretical
tendency of Pb*2 to corrode in this pH?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2 is 1.00 atm, calculate the cell potential at 25.0°C.
At 298 K a cell reaction has a standard emf of +0.18 V. The equilibrium constant for the cell reaction is 6.1×105. A. What is the value of n for the cell reaction?
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?
Please don't provide handwritten solution...
17. Calculate the cell potential of the cell described below: 2+ Al(s) | Al³+ (aq) (1.00 M) || Pb²+ (aq) (1.00 M) | Pb(s)
A cell consisting of two silver plates dipping in a 0.1 M and 0.01 M solution of silver nitrate AgNO3 respectively at 25 °C. 1- diagram the cell, 2- write the cell reaction 3- Calculate the cell potential
What is the standard cell potential for a galvanic cell that consists of Au3+/Au and Ni2+/Ni half-cells?Identify the oxidizing and reducing agents.
A student does an experiment to determine the molar solubility of magnesium fluoride. She constructs a voltaic cell at 298 K consisting of a 0.713 M magnesium nitrate solution and a magnesium electrode in the cathode compartment, and a saturated magnesium fluoride solution and a magnesium electrode in the anode compartment. If the cell potential is measured to be 8.13×10-2 V, what is the value of Ksp for magnesium fluoride at 298 K based on this experiment? Ksp for MgF2 = ------
Determine the cell potential (E) from the following half-cells: Pbo/Pb2+ and Zno/Zn2+ where [Pb2+] = .86M and [Zn2+] = 0.35 M. Calculate K for this reaction. How long in hours would you have to let it go until you lower the voltage to 85 percent of the E from the Nernst equation at 7.2 amps?
Silver (Ag) is observed to corrode in HCl (1M activity) in aerated condition. 1) Write the anodic and cathodic half reactions. Write ½ reactions as reduction reactions. 2) What are the standard potentials of the ½ reactions