Fig. 8Select one:O +1.66 V-1.66 V+0.16 V+3.16 VAuThe value of the standard cell potential of the cell in Fig. 8 is calculated to beFig. 9Use the following information to answer the next question.The following three open systems were set up to study corrosion and corrosion preventionAFe-neilB1.0 mol/L HCI 1.0 mol/L AI(NO),с1.0 mol/L, KNO,Beaker ASalWaterBeaker Results after 48 hoursProcessBeaker B-Al(s)SanWaterIdentify the results of each system in figure 9 after they are allowed to sit for 48 hours. For each beaker, indicate whether the iron nail will exhibit corrosion.Painting the pipe•-Fe nail wrappedin a strip of Zn•Beaker CWhich of the following would protect an iron pipeline from rusting?Connecting it to a low voltage power supplyBaltWolorConnecting the pipeline to electrodes made of copper.-Fe naill wrappedin a strip of CuImmersing the pipe in a silver nitrate solutionProtection from corrosion+

Answered: Image /qna-images/answer/06244fcb-345a-4a9b-8c6c-d5b4f6f8e889.jpg

Answered: Fig. 8 Au 1.0 mol/L KNO, O-1.66 V O…

Fig. 8 Au 1.0 mol/L KNO, O-1.66 V O +0.16 V +3.16 V of 1.0 mol/L HCI Al(s) 1.0 mol/L AI(NO), The value of the standard cell potential of the cell in Fig. 8 is calculated to be Select one: O +1.66 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: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd2+ + 2 e Cd (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: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The call reaction at anode is, H2(g) ------> 2H+(aq) + 2e- Standerd cell potential of the cell =…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

A: Given that, an electrochemical cell is Cus|Cu2+0.11 M||Fe2+0.0063 M|Fes. Also, the standard…

Q: your answer in the provided box. A constant current is passed through an electrolytic cell…

A: Given,produced volume of Cl2 gas at anode ( at STP ) = 4.18 Ltime taken = 16 h.

Q: Your mystery voltaic cell has a standard cell potential of 0.741 V and can be written in cell…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: A voltaic cell employs the following redox reaction: 2Fe^3+(aq)+3Mg(s)→2Fe(s)+3Mg^2+(aq) Calculate…

Q: Starting with a cell described below: Al | Al3+ (1.00 M) || Pb2+ (1.00 M) | Pb What is the cell…

A: In this question we have to calculate the cell potential of following happen in enough time to…

Q: A student is given two beakers in the laboratory. One beaker contains a solution that is 0.14 M in…

A: Given: [Mn3+ ] = 0.14 M [Mn2+ ] = 0.46 M [Sn2+ ] = 0.28 M And [Sn4+ ] = 0.056 M

Q: Determine the standard cell potential, E°cell, for a galvanic cell that employs the half-reactions :…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The Nernst equation is a mathematical relationship used in electrochemistry that relates the…

Q: Calculate the maximum cell potential under these conditions. Show your work. Ecell = (round to 2…

A: we have to calculate Ecell

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given Ecell = 0.233V Ecell = - RTnFln [H+]0.233= - 8.314 x2981 x 96500ln [H+]- 9.075 = ln [H+] [H+]…

Q: The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76…

Q: The standard reduction potential of Cu(s) is + 0.339 V. What is its standard oxidation potential?…

Q: (c) The magnitudes but not the signs of the standard electrode potentials of two metals, X and Y…

A: In this given question we have to find out standard emf of a cell made up of X and Y metal.

Q: Use the References to access important values if needed for this question. Use standard reduction…

A: " Since you have posted multiple questions, we will provide the solution only to the first question…

Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) →Mn²+(1.00 M) + H₂(g)(1.00 atm) If the cell…

A: Given,The cell reactions:

Q: When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 94.68 °C with the…

Q: Zn+2{ag) + Ni(s) For the reaction : Zn (s) + Ni*2(ag) → Ni*2 (ag) = 0.50 M Znr2 (ag) = 0.76 M The…

A: Interpretation : We have to tell the cell potential; for the given cell.

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: What does a negative standard cell potential imply about the reaction?

A: The potential difference between the cathode and anode half cell under the standard conditions of…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given Ecell =0.189we know E°cell is 0 for hydrogen cell.

Q: Consider compounds A-D, which contain both a heteroatom and a double bond. H. A D a. For which…

A: Resonance structure:If the Lewis structure of a molecule or ion cannot explain by a single structure…

Q: A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at…

A: Given: Time passed = 31.5 hr = 31.5 × 3600 = 113400 s (Since 1 hr = 3600…

Q: The galvanic cell test setup given in the figure is at 25 ° C. It Show the total reaction by writing…

A: Oxidation occurs at anode. Hence, Zn (s) --> Zn2+ (aq) + 2 e ...(1) Reduction…

Q: If the standard voltage of the reaction of Cu(s) with Ag*(aq) is 0.46 V, what is the standard gibbs…

Q: H. H. CH3 HO H O Saturated Fatty Acid O Unsaturated Fatty Acid OTriglyceride O Glycerol

A: Fatty acids are the organic compounds present in the cell membranes, mainly in the lipid layer. The…

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.20 M and [Pb2+] =…

A: Equilibrium constant can be defined as the ratio of concentration of products to concentration of…

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M)=Cd²+(1.00 M) + H₂(g)(1.00 atm) If the cell…

A: The cell reaction given is, Given: Cell potential = 0.168 V And temperature = 298 K

Q: A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at…

A: Cell delivers = 0.31 A or 0.31 C/sec In 1 sec charges delivered = 0.31 C 32.1 hr = 3600 sec × 32.1…

Q: sing the following standard reduction potentials Fe3+(aq) + 2e- = F2+(aq)…

A: The given half cell reactions along with their standard reduction potentials are given as follows:…

Q: Consider the electrochemical cell reaction of hydrogen gas and chlorine gas to produce 1 mol of HCI…

Q: If the coefficients of a balanced reaction are all multiplied by 2, the cell potential is also twice…

A: Given that we have to multiply the coefficient of a cell reaction with 2.

Q: What is the cell potential of the following cell at 25 oC? Ni(s) | Ni2+ (1.0 M) || Sn2+…

A: The cell reaction taking place is Ni (s) + Sn2+ (aq) ----> Sn (s) + Ni2+ (aq) Hence the…

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: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: Given, The voltaic cell, Zn2+ - Zn When the two half-cells have [Zn2+] = 1.8 M and[Zn2+] = 1.00…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Fig. 8
Select one:
O +1.66 V
-1.66 V
+0.16 V
+3.16 V
Au
The value of the standard cell potential of the cell in Fig. 8 is calculated to be
Fig. 9
Use the following information to answer the next question.
The following three open systems were set up to study corrosion and corrosion prevention
A
Fe-
neil
B
1.0 mol/L HCI 1.0 mol/L AI(NO),
с
1.0 mol/L, KNO,
Beaker A
Sal
Water
Beaker Results after 48 hours
Process
Beaker B
-Al(s)
San
Water
Identify the results of each system in figure 9 after they are allowed to sit for 48 hours. For each beaker, indicate whether the iron nail will exhibit corrosion.
Painting the pipe
•
-Fe nail wrapped
in a strip of Zn
•
Beaker C
Which of the following would protect an iron pipeline from rusting?
Connecting it to a low voltage power supply
Balt
Wolor
Connecting the pipeline to electrodes made of copper.
-Fe naill wrapped
in a strip of Cu
Immersing the pipe in a silver nitrate solution
Protection from corrosion
+

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: Introduction

VIEW

Step 2: Cathode and anode

VIEW

Step 3: Calculation of the standard cell potential

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 4 images

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

Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.216 V, what is the pH of the unknown solution at 298 K? pH =
Consider the following cell reaction: Fe(s) + 2 H"(? М) —Ғе*"(1.00 М) + H-(g)(1.00 atm) →Fe? If the cell potential at 298 K is 0.164 volts, what is the pH of the hydrogen electrode? pH
Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP"(1.00M) | Pb³"(1.00M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al"] to have changed by 0.60 mol/L. (Assume T = 25°C.) (b) Many elements have been synthesized by bombarding relatively heavy atoms with high-energy particles in particle accelerators. Complete the fol- lowing nuclear equations, which have been used to synthesize elements. U + C-→ Cf + Cf + 'B Lr + + He Bk + in + 6 n 10 Db + 4 in 103
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.
How long (in hours) must a current of 5.0 amperes be maintained to electroplate 60g of calcium from molten CaCl2?
A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.
1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential 2) Calculate the free energy change and the cell potential for the reaction at 298.0 K if all reactants are at 2.00 M and/or 2.00 atm and all products are at 0.0100 M and/or 0.0100 atm
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ( PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.201 V, what is the pH of the unknown solution at 298 K? pH =
Use the tabulated half-cell potentials to calculate ΔG° for the following reaction. (Hint: Before you being, you must determine whether or not the reaction is balanced.)I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq) (a)‒1.1×102kJ (b) +4.9×101kJ (c) ‒9.7×101kJ (d) ‒3.3×102kJ