For the reaction : Als) / Al® aq) // Mg*?«aq) / Mg(s) the amount of cell potential produced is and is a reaction. O +0.71 spontaneous -0.71 V non-spontaneous O +2.15 V spontaneous -2.15 V non-spontaneous

For the reaction : Als) / Al® aq) // Mg*?«aq) / Mg(s) the amount of cell potential produced is and is a reaction. O +0.71 spontaneous -0.71 V non-spontaneous O +2.15 V spontaneous -2.15 V non-spontaneous

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 cell potential of this electrochemical cell depends on the gold concentration in the cathode…

Q: What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0205 V and n =…

A: The objective of the question is to calculate the equilibrium constant (K) for an electrochemical…

Q: Given that E = 1.88 V. calculate the standard Gibbs energy for the cell at 25 °C. O 538 kJ mol O…

A: Given: E°cell = 1.86 V

Q: Calculate the emf at 298 K generated by a voltaic cell in which the reaction isCr2O72-(aq)+ 14…

Q: Calculate values for the galvanic cells desch (a) Cr³+ (aq) + Cl₂(g) = Cr₂0,2 (aq) + Cl(aq) V (b)…

Q: give proper explanation.

A: The objective of this question is to calculate the change in Gibbs free energy (ΔG°) for the given…

Q: The voltaic cell (represented by notation A) will produce a greater magnitude of negative Gibbs free…

A: Here we have to predict which Galvanic cell have greater magnitude of Gibbs free energy . The…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -7.4 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

Q: The following reaction is spontaneous as written when the components are in their standard states:…

A: Answer:Galvanic cell is a type of cell that converts chemical energy into electrical energy via…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -4.5 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

Q: The following electrochemical notation represents correctly the spontaneous concentration cell for…

Q: ΔGo Eo K a 24kJ b 0.120V c 0.114 Consider a cell reaction at 25oC where n=3. Fill in the…

A: The relation between standard Gibbs free energy and standard cell potential for a reaction is as…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -5.9 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

Q: Calculate E°ell for the cell schematic as written: Fe(s) | 1M FeCl, (aq) || 1 M AI(NO,)o (ag) | Al…

A: The cell given is .

Q: Calculate the value of the cell potential, Ecell, for this reactión at 29 [1"] = 0.0050 M, and [Br2]…

A: In the given cell reaction, iodine is reduced and bromine is oxidized. The standard oxidation…

Q: The standard EMF for the cell using the overall cell reaction below is +0.80 V: 2AI (s) + 312 (s) →…

Q: A certain metal M forms a soluble sulfate salt M, (SO4), Suppose the left half cell of a galvanic…

Q: The standard cell notation for the following redox reaction is 2 Al(s) + 3 F₂ (g) → 2 A1³+ (aq) + 6…

Q: Calculate the standard Gibbs free energy change, AG°, at 25 C for the following reaction. E°cu"/cu =…

Q: Tempjetes Symbo Gibbs energy change, ArG", is related to cell potential, Ee. by the equation A,G" =…

A: Part A: Answer: ∆rG° = -372 kJ/mol

Q: Consider the reaction in the lead-acid cell Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(aq) + 2H2O(l) for…

A: Given information: E°cell = 2.04 V Temperature = 298 K The reaction is given as follows: Pb(s) +…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -3.9 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: Given- ∆G°= -3.9kJ/mol = -3900 J/mole (1KJ = 1000J) n=3 F=96500 J/(V.mol)

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

Q: Which of the following is not a sufficient condition for a spontaneous process? ΔG 0 ΔE 0(cell) >…

A: A process which proceed in the forward direction without doing anything from outside, or without any…

Q: nitrate, Ni(NO3)2 undergoes electrolysis in order to plate on a sink faucet requiring 2.00 hours…

A: Given, Time(t) = 2.0 hrs = 7200 seconds Current(i) = 2.80 amp Faraday's constant(F) = 96, 485…

Q: The E° for the following cell at 298 K and 308 K are 0.058V and 0.0614V respectively. What is the…

A: Given cell reaction consisting of anode and cathode half-reaction can be represented as: Ag(s)…

Q: What is the cell potential (in V) for the reaction below with the given concentrations at 33.0 oC?…

A: Given concentrations:[H+] = 0.152 M[NO3- ] = 0.470 M[Fe3+ ] = 0.885 M[NO] = 0.623 MFirst, let's…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V Sn2*(aq) +…

A: Species with higher Ereduction value are the strongest oxidizing agent and weakest reducing agent.…

Q: Consider the given reaction of mercury (II) oxide being reduced to liquid mercury. If 0.3 amperes…

A: We can calculate weight by using Farady's law of electrolysis W = EIT÷ F Where E = equilivalent…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -5.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: The objective of this question is to calculate the standard cell potential (E°) for a galvanic cell…

Q: cell potential

Q: Consider the voltaic cell with a standard cell potential of 2.89 V: Sr(s)|Sr²+ (1.0 M)||H* (1.0…

Q: Determine if the following reaction is spontaneous in standard conditions Cl'(ag) + 4MNO2(6) +…

A: Given reaction is : Cl- (aq) + 4MnO2 (s) + 8H+ (aq) -----> ClO4- (aq) + 4Mn2+ (aq) + 4H2O (l)…

Q: (16) Consider the following redox reaction that occurs in an electrochemical cell: Fe²+ (aq) + Al(s)…

A: 16) Given, Fe2+(aq) + Al(s) ➝ Fe(s) + Al3+(aq) Standard gibbs free energy (∆G°) = ? Standard…

Q: For the galvanic cell, C(gr) | Cs(s) |Cs*(aq) || Sn²*(aq) | Sn(s), what is the function of the…

Q: Given the reaction: 2 H₂O(l) → 2 H₂(g) + O₂(g) for which AH°25°c = +571.7 kJ. Determine the cell…

A: 2H2O(l) = H2(g) + O2(g) Required cell representation Reaction at cathode : O2 + 2H2O + 4e- = 4OH-…

Q: Half-reaction E° (V) I2(s) + 2e→ 21I(aq) 0.535V Pb"(aq) + 2e → Pb(s)|-0.126V Zn-(aq) + 2e →…

A: Since you have asked a question with multiple subparts, we will answer only first three subparts for…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -6.6 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: ∆G°= -6.6 kJ/mol = -6.6×103 J/mol n = 3 F = 96500 J/V.mol E°=?

Q: 4) Determine cell potential, at 298 K, for the following cell if the copper ion concentration is…

A: The electrochemical cell described involves a redox reaction between copper (Cu) and iron (Fe)…

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V PH2=0.857atm Concentration of Cd2+=1.00M

Q: Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: The free energy change for the following reaction at 25 °C, when Cr³+ = 1.20 M and Zn²+ 2Cr³+ (1.20…

A: In the question, the reaction isWe need to find for this reaction. and

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -6.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: Given, ∆G° = -6.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol) □G° = -nFE°

Q: Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F°(aq) 2.870V 2+ Pb"(aq) +…

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

Q: What is the equilibrium constant K at 25.0 °C for an electrochemical cell when E° = +0.120 V and n =…

A: Given,The standard cell potential ( Eo ) =+0.120 VNumber of moles of electrons (n) =2( F…

Q: 3. Assuming standard states for all reactants and products, determine the spontaneous direction of…

A: The reactions given are, 1) Cu + 2 HCl → CuCl2 + H2 2) Ag + FeCl3 → FeCl2 + AgCl

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -3.3 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: The question is based on the concept of electrochemistry. we have to calculate standard reduction…

Question

For the reaction : Als) / Al® aq) // Mg*?«aq) / Mg(s) the amount of cell potential produced is
and is a
reaction.
O +0.71 spontaneous
-0.71 V non-spontaneous
O +2.15 V spontaneous
-2.15 V non-spontaneous

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

Step 2

Step 3

Step 4

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 certain metal M forms a soluble sulfate salt M,SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 22.5 mM solution of M,SO, and the right half cell with a 4.50 M solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 25.0 °C. O left Which electrode will be positive? O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Consider the following galvanic cell: Agls) | Ag"(3.0 x 104 M) || Fe3"(1.1 × 10³ M), Fe²"(0.040 M) | Pt(s) Choose the correct cell potential. O Ecel - - 0.12V Ecell = + 0.09 V O Ese = - 0.15 V O Eçel = + 0.12 V eTextbook and Media Hint Determine the sign of the electrodes in the cell. The left side half-cell is the v and charged. The right side half cell is the v and charged. Enter the equation for the spontaneous cell reaction. (Enter states of matter in your answer.)
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br°(aq)||1.080V 2+ Sn"(aq) + 2e - → Sn(s) ||-0.140OV 2+ Zn"(aq) + 2e¯ →Zn(s)|-0.763V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Zn(s) reduce Br2(1) to Br (aq)? (6) Which species can be oxidized by Sn2*(ag)? If none, leave box blank.
Chemistry 19.10.-Calculate the standard potential, ,E°, for this reaction from its AG° value. X(s)+Y4+(aq)-X4+(aq)+Y(s) AG•=31.0 kJ
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
Calculate the Gibbs free energy (AG°) of the reaction below. Is this reaction spontaneous or nonspontaneous? Ag (s) + Fe*(aq) = Ag* (aq) + Fe2*(aq) E° (V) 3+ Fe *(aq) + e Fe2"(aq) 0.77 Ag +e Ag(s) 0.80 A/
Calculate ΔG° for the following balanced redox reaction and determine if the reaction is spontaneous. (values are made-up) 2 Na+(aq) + 2 Cl-(aq) → 2 Na(s) + Cl2(s) Na+(aq) + e⁻ → Na(s) E° = +0.362 V Cl2(s) + 2 e⁻ → 2 Cl-(aq) E° = +0.789 V use this equation: Δ G ° = − n F E cell °
What is Keq at 298 K for the spontaneous reaction between the following?Pb+2 (aq) + 2e-------> Pb (s) Eo = -0.13 VMn+2 (aq) + 2e-------> Mn (s) Eo = -1.18 V
Determine E° for a galvanic (voltaic) cell if ∆G° = -6.3 kJ/mol and n = 3. (F = 96,500 J/(V･mol))
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Calculate E for the following unbalanced reactions. Indicate if the reactions are spontaneous as written. (a) Al3+(aq) + Mg(s) → Al(s) + Mg2+(aq)(b) ClO4-(aq) +Mn2+(aq) + H2O(l) → MnO4-(aq) + H+(aq) + ClO3-(aq) Given data:Al3+ + 3e-→Al Ered =-1.66 v Mg2+ + 2e-→Mg Ered= -2.37 vMnO4- + 8H+ +5e-→Mn2+ + 4H2O Ered= 1.51 v ClO4- + 2H+ +2e- →ClO3- + H2O Ered= 1.19 v
Use Table to determine whether the following reactions are spontaneous under standard conditions.(a) Cu(s) + 2 H+(aq)---->Cu2+(aq) + H2(g)(b) Cl2(g) + 2 I-(aq)---->2 Cl-(aq)+ I2(s)