Answered: Asuming these half reactions make a…

Asuming these half reactions make a galvanic cell, what is the cell potential in volts. E F2 (g) + 2e →F (aq) Al3+ + 3e- → Al(s) = 2.87 %3D red E. -1.66 red 2,265

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.19QAP

See similar textbooks

Related questions

Q: For each of the two electrochemical systems below write each half reaction and then calculate the…

A: Here we have to determine Ecell of the following cell reaction. For this we have to apply Nernst…

Q: For the reaction 2FE3+ (aq) + Sn 2* (aq) → Sn 4* (aq) + 2Fe 2* (aq). at 25 °c, Calculate (using the…

Q: A galvanic cell is constructed in which the overall reaction is Cu(s) Cu²+ Br2 Br¯ It is found that…

Q: Consider a spontaneous concentration cell based on the following half-reactions (where "a" stands…

Q: A voltaic cell is constructed from a standard Sn?*|Sn half cell (E°red = -0.140V) and a standard F,F…

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential (Eᵒcell)…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e- →…

A: We have two half cell reaction: X3+ + 3e- ----> X(s) E°= -1.61 V Y3+ + 3e- ---->…

Q: 2. Consider the cell reaction: MnO4 + Fe* → Mn²* + Fe³* SRP: E° Fe*/Fe2* = +0.77 V; E° MnO,/Mn²* =…

Q: Given the balanced redox reaction equation for a galvanic cell as below. Mg(6) + 2 Ag" (ag) → Mg…

A: We have 0.01 M Ag+ 0.15 M of Mg+2, we have to predict shorthand notation ,cell potential and predict…

Q: A galvanic cell is constructed of two half cells Zn2+*(aq)/Zn(s) and H2(g)/H*(aq) separated by a…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: The redox reaction below has a AG value of 219. kJ. Determine the standard cell potential (Eᵒcell)…

Q: The oxidation of hydrogen by oxygen is one of the most-used reactions in fuel-cell technology. The…

A: The relationship between the E0cell and ΔG0 is given by nFE0cell = -ΔG0 where n = number of…

Q: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

A: Given reaction: 2 Fe2+ (aq) + H2O2 (aq) + 2H+ (aq) → 2 Fe3+ (aq) + 2 H2O (l) It is given that all…

Q: 5) In an electrochemical cell, Cu(s) is placed in the anode half-cell while Ag(s) in the cathode…

Q: a. How many grams of NaCl is required to generate a 0.50 L 3.00M NaCl (aq) solution? b. Calculate…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Calculate E°cell for the unbalanced redox reaction A(s) + B+(aq) → A2+(aq) + B(s) given the…

Q: Consider the following two oxidation potentials. Determine the spontaneous Ecell that would result…

A: We know, higher the oxidation potential, the higher will be its ability to get oxidized. The…

Q: What is the standard electrode potential for a galvanic cell constructed in the appropriate way from…

A: Metal having high reduction potential acts as cathode. But metal having low reduction potential acts…

Q: A galvanic cell is set up using the redox reaction below at 298 K. If the cell has a standard cell…

A: In a galvanic cell, the Gibbs free energy is related to standard cell potential as,…

Q: Consider a galvanic cell with the following half-reactions: MnO4– + 8 H+ + 5e– → Mn2+ + 4 H2O…

A: Given half cell reactions are : MnO4– + 8H+ + 5e– → Mn2+ + 4H2O , E° = 1.51…

Q: Given the balanced electrochemical reaction below (M and N represent generic metals), what is the…

A: Welcome to bartleby ! Introduction : We have to calculate E° cell

Q: Upload a picture (*.png, *.tiff, *.tif, * pdf. *.jpg) of your hand-written work in response to the…

A: a.) Write the expression for change in standard Gibbs free energy of reaction in terms of standard…

Q: Using the equation Esell = E°sathode- E°anode, calculate the overall cell potential for the cell in…

A: Interpretation: We have to write the naming for the following .

Q: What is E° for the cell Mn | Mn²⁺(aq) || Ag⁺(aq) | Ag?

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

Q: A voltaic cell is constructed from a standard AgAg half cell (E°, red = 0.799V) and a standard F2F…

A: We have given that Ag+/Ag E°red = 0.799 V F2/F- E°red = 2.870 V

Q: For cell schematic notation Zn(s) | ZnCl2 (1.0 M )| | CuSO4 ( 2.0 M ) | Cu(s)…

Q: Consider the following two oxidation potentials. Determine the spontaneous Ecell that would result…

A: Nernst equation is used to calculate the reduction potential of electrochemical cells. Oxidation…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e → X(s)…

Q: voltaic cell is constructed from a standard Ni2+|Ni half cell (E°red = -0.250V) and a standard…

A: Hg+2/Hg=0.855ev it will go to cathode electrode because it have highest electrode potentail Rxn is…

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: The redox reaction below has a AG value of 230. kJ. Determine the standard cell potential(Eᵒcell)…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e- X(s)…

A: The solution is as follows :

Q: Consider these two entries from a fictional table of standard reduction potentials. X+ +3e X(s) E° =…

A: To calculate E°Cell identify cathode and anode.

Q: Consider the reaction: A3+ (aq) + B(s) → B3*(aq) + A(s) The standard electrode potential of the…

A: a) answer: ∆G° = 272 kJ/ mol

Q: Li(s)|Li+ (aq,1 M)||Zn2+(aq, 1 M)|Zn(s) A.Write half-reactions occurring in the electrochemical…

Q: Consider the following half-reactions: I2(s) + 2e- → 2 F(aq), E°(red) = 0.54 V, Cd²"(aq) + 2 e- →…

A: In a galvanic cell spontaneous reaction occurs. In a electrolytic cell non-spontaneous reaction…

Q: 26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e -->…

Q: Consider a galvanic cell with the following half-reactions: MnO4-+ 8 H†+5e¯ → Mn²+ + 4 H2O E° = 1.51…

A: The answer are as follows:

Q: Consider the galvanic cell based on the following half-reactions: Zn+ +2e Zn e =-0.76 V Fet + 2e Fe…

Q: 4. Assume that you have 0.001 Fe* and 0.002 Fe2* (i.e., the solution contains Ferrous and Ferric…

A: In a model cell there are two electrodes one is cathode and another one is anode. In cathode…

Q: Consider the galvanic cell based on the following half-reactions: + 2e + Zn e° = -0.76 V Cd²+ + 2e →…

A: Given : Zn+2 + 2e- -----> Zn E° = -0.76 V Cd+2 + 2e- ------> Cd E° = -0.40 V

Q: 19. Calculate standard potential of the cell made out of Zn/Zn2+ and Fe/Fe2+ half- cells. Standard…

A: The standard potential of cell can be determined from Nernst equation. The reaction will be…

Q: Given the balanced electrochemical reaction below (M and N represent generic metals), what is the…

A: A cell's standard state potential is the potential of the cell under standard conditions, i.e.…

Q: Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their…

Q: A nonstandard cell or half-cell potential can be calculated using the Nernst equation: RT InQ nF E=…

A: Ans.

Q: How many grams of NaCl is required to generate a 0.50 L 3.00M NaCl (aq) solution?

A: Since you have posted multiple questions, we will solve only first question for you. If you want…

Q: AG", rzn =-474 kJ/mol Electrode Half-Reaction Standard Reduction Cathode O2(9) + 4 H* (aq) + 4 e → 2…

Q: A lithium battery is being developed. Its voltaic cell is constructed based on Li metal electrode…

A: We are given standard reduction potential values of two different half cells:

Question

this is wrong, please give me correct answer!!!!

Asuming these half reactions make a galvanic cell, what is the cell
potential in volts.
E
F2 (g) + 2e →F (aq)
Al3+ + 3e- → Al(s)
= 2.87
%3D
red
E.
-1.66
red
2,265

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Selection Rules for Pericyclic Reactions

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

Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni