Calculate E°cell for a copper-aluminum cell in which the cell reaction is:AI3* (aq) + 3Cu(s)Al(s) + 3Cu* (aq)A3*(aq) + 3eAl(s) E° = -1.66 V%3DCu*(aq) + e¯Cu(s) EO = 0.48 VO a. 2.2 VO b.-1.18 VOC. 1.18 VO d. 2.14 VO e. 2.14 V

Answered: Image /qna-images/answer/c8d4e7ad-b9c2-4212-8998-c09766401329.jpg

Calculate E°cell for a copper-aluminum cell in which the cell reaction is: AI3* (aq) + 3Cu(s) Al(s) + 3Cu*(aq) Al3*(aq) + 3e Al(s) E° = -1.66 V %3D Cu* (aq) + e¯ Cu(s) EO = 0.48 V O a. 22 V O b.-1.18 V OC. 1.18 V O d. 2.14 V O e. 2.14 V

Calculate E°cell for a copper-aluminum cell in which the cell reaction is: AI3* (aq) + 3Cu(s) Al(s) + 3Cu(aq) Al3(aq) + 3e Al(s) E° = -1.66 V %3D Cu* (aq) + e¯ Cu(s) EO = 0.48 V O a. 22 V O b.-1.18 V OC. 1.18 V O d. 2.14 V O e. 2.14 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: If a redox reaction occured with the 2 redox couples provided below, which species would be the…

A: Reducing agent is the substance that reduces the other species and itself gets oxidized.

Q: Balance the following redox reaction in acidic aqueous solution: 2I-(aq) + Cr2O72-(aq) -> I2(s) +…

A: 2I-aq+Cr2O7-2aq→I2s+2Cr+3aq stepI split the equation in to half reaction…

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

A: We have to find ∆G, ∆E and K for given reaction And using given reduction potential of half cell

Q: equilibrium constant

Q: Consider the following half-reactions: Cl2(9) + 2e - 2cF (ag) = 1. %3D I2(9) + 2e - → 21 (aq) E, =…

A: From given data , based on the E° value given for the half actions we can predict the strongest…

Q: The reduction potential for Ag +(aq) is +0.800 V and for MnO 4 -(aq) is +0.60 V. The reaction below…

Q: Consider the following cell. Cr | Cr³+ (1.00 M) || Ni²+(1.00 M) | Ni = 0.68 V (a) How many…

A: (b) Write the balanced chemical equation for the overall cell reaction and use the ICE table.

Q: The equation AG = -nFE also can be applied to half-reactions. Use standard reduction potentials to…

Q: A concentration cell based on the following half reaction at 288 K Ag +e Ag; SRP = 0.80V is made…

A: Reaction on L.H.E.: Ag(s) ⇌Ag+(0.354M) + e- A⏜A (oxidation) Reaction on R.H.E. Ag+(1.4 M)+e-⇌Ag(s)…

Q: Question 5, Part d: How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum…

Q: Given the half-cell reduction potentials, the overall cell reaction, and cell potential below:…

A: Dear student I have given answer to your question in the image format

Q: 24. The following redox reaction is spontaneous as written: Ca2+(aq) + Zn(s) ⟶⟶ Zn2+ + Ca(s)…

A: Given, Chemical Reaction : Ca2+(aq) + Zn(s) ⟶⟶ Zn2+ + Ca(s)

Q: What is the cell potential given the balanced redox reaction? 2+ Mg6) + Cu?+ → Cu(s) + Mg“ (aq) (aq)…

A: The answer to the following questions is-

Q: The free energy change for the following reaction at 25 °C, when [Cu²+] = 3.44×10-3 M and [Cu²*] =…

Q: Use the data from the redox table (appendix L in the text) to calculate equilibrium constants for…

A: Given- Reaction Ag2S (s) <=> 2 Ag(s) + S2- (aq) Temperature = 298.15 K To find- Equilibrium…

Q: (a) Calculate ArG° for the reaction:Mg(s) + Cu22+(aq) > Mg2+(aq) + Cu(s)Given: E°cell = + 2.71 V,…

A: (a) The given reaction is, E◦ cell = 2.71 V Number of electrons transferred, n = 2 1 F = 96500…

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

A: Recall the given reaction, From the ALEKS Data tab,The…

Q: Given the standard reduction potentials: Ce+ + e – Ce³+ +1.61 v K* + e° → K -2.93 v The strongest…

A: GivenCe4+ + e- → Ce3+ = +1.61 VK+ + e- → K = -2.93 VStrongest…

Q: Refer to the list of standard reduction potentials below. Which species will react spontaneously…

Q: An alcohol or an alkane? Why? An ether or an aldehyde? Why? A ketone or a carboxylic acid? Why?…

A: Good evening. Thank you, Hope this helps!Explanation:Approach to solving the question: Detailed…

Q: Based on the reduction potential data below for two metals, what is the standard cell potential for…

A: The overall reaction is as folllows: Dy(s) + Ho2+(aq)→Dy2+(aq) + Ho(s). Since the reduction…

Q: A cell employs the following half-reactions. Ni(s) Eº2+ = -0.25 V Cr(s) E°3+ = -0.74 V Ni Calculate…

A: Given, Ni2+(aq) + 2e- ----> Ni(s) E°Ni2+ = -0.25 V Cr3+(aq) + 3e- -----> Cr(s) E°Cr3+ = -0.74…

Q: Calculate the pK for the oxidation of X by Hplus at 25 degrees C. X(s) + 1 Hplus → X1 plus (aq)+…

Q: 8. Calculate Eº, E, and AG for the following cell reactions: (a) Mg(s) + Sn²+ (aq) → Mg²+(aq) +…

Q: For the following balanced redox reaction in acidic solution: 3 Sn4+ + 2 Au(s) → 3 Sn²+ + 2 Au³+…

A: Sn4+=0.63 MSn2+=8.2×10-3 MAu3+=6.9×10-5 M

Q: Use the standard reduction potentials, please calculate the AE and determine the spontaneity (AG > 0…

Q: Consider the following reaction: MnO4 (ag) + 5FE2+ + 8H (aq) - Mn2+ (aq) + 5FE3+ (aq) + 4H2O) (aq)…

Q: The free energy change for the following reaction at 25 °C, when [Cd²+]= 9.77×10-3 M and [Cu2+] =…

Q: Consider the following redox half-reaction at 25 °C: MnO4 (aq) + 8 H* (aq) + 5 e¯ → Mn²* (aq) + 4…

Q: When [Cu2+] = 1.24 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: The overall cell reaction : Cu2+(aq) + Zn(s) ---> Cu(s) + Zn2+(aq) The observed cell potential…

Q: 6. Consider the following reaction: 2Fe²⁺(aq) + Cu²⁺ → 2Fe³⁺(aq) + Cu. When the reaction comes to…

A: Given, The reaction: 2Fe²⁺(aq) + Cu²⁺ → 2Fe³⁺(aq) + Cu. When the reaction comes to equilibrium, the…

Q: Using the reduction potentials given, calculate the equilibrium constant, K, at 25°C for the…

A: Electrochemical cell is a cell in which electrical energy is converted to chemical energy.

Q: 10. Use the standard reduction potentials, please calculate the AE and determine the spontaneity (AG…

Q: Use the standard reduction potentials located in the "Tables' linked above to calculate the standard…

Q: Use standard reduction potentials (shown below) to calculate the potential of a nickel- cadmium cell…

Q: The standard reduction potential E° for the reduction of permanganate in acidic solution is +1.51 V.…

A: Given, E° for reduction of permanganate in acidic solution is +1.51 V. We have to calculate the…

Q: Consider the following reduction half-reactions: MnO4 (aq) + 8 H*(aq) + 5 e¯ = Mn²+ (aq) + 4H₂O(1)…

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: Voltage can be calculated as follows

Q: Given the following standard reduction potentials: Mg2 (aq) + 2e - Mg(s) E° = -2.357 V %3D Al3* (aq)…

A: We have to predict the spontaneous reaction.

Q: For the cell diagram below, what is the equilibrium constant K for the reaction at 25 °C? * Pt(s) |…

A: We are given a cell notation of an electrochemical cell. With standard reduction potential values of…

Q: Calculate the cell potential for the following reaction and indicate whether it is spontaneous or…

Q: Use the appropriate standard reduction potentials below to determine the equilibrium constant at 386…

A: E°cell = E°red cathode - E°red anode here anode is Fe because it has less reduction potential and…

Q: Cr3+(aq) + 3e- à Cr(s) -0.763 V Au+(aq) + e- à Au(s)…

A: Given reactions are : Cr3+(aq) + 3e- -------------> Cr(s) E0 = -0.763…

Q: The equilibrium constant, Kc, was found to be 1.4 x 10 at 25.8°C for th ction, 2X[s)+ Cu (aq)-->…

A: Given: Kc is 1.4×103. Temperature is 25.8oC. Reactions: Cu2+(aq)+2e-→Cu(s) Eo+0.30 V To find:…

Q: Using the following standard reduction potentials, e*(aq) + e¯ → Fe²*(aq) Ni2*(aq) + 2 e →Ni(s) E° =…

A: The electrochemical cell that utilizes energy released from a spontaneous chemical reaction to…

Question

Calculate E°cell for a copper-aluminum cell in which the cell reaction is:
AI3* (aq) + 3Cu(s)
Al(s) + 3Cu* (aq)
A3*(aq) + 3e
Al(s) E° = -1.66 V
%3D
Cu*(aq) + e¯
Cu(s) EO = 0.48 V
O a. 2.2 V
O b.-1.18 V
OC. 1.18 V
O d. 2.14 V
O e. 2.14 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

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

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 the following standard reduction potentials. O₂(g) + 2H₂O(1) +4 Ca²+ (aq) +2e - 40H (aq) E° = 0.401 V Ca(s) E= -2.868 V E°
Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced Half-Reaction E°(V) MnO4 (aq) + 3e MnO2(s) (at basic pH) 0.59 Fe3+(aq) + e- Fe2*(aq) 0.77 What is the balanced reaction taking place in the cell (in basic solution)? 2 H20(1) + Mn04 (aq) + 3 Fe3+(aq) → 3 Fe2*(aq) + MnO2(s) + 4 OH- MnO2(s) + 4 OH¯ + 3 Fe3+(aq) 3 Fe2+(aq) + 2 H20(1) + MnO4¯(aq) MO 3 Fe2*(aq) + 2 H2O(1) + MnO4¯(aq) MnO2(s) + 4 OH¯ + 3 Fe3+(aq) M 3 Fe2+(aq) + MnO2(s) + 4 OH → 2 H20(1) + MnO4 (aq) + 3 Fe3+(aq)
Plese don't provide handwritten solution
Consider the following reaction and standard reduction potential data. 2Ag (aq) + Cu(s) 2Ag(s) + Cu*"(aq) Half reaction E°(V) Ag (aq) +eAg(s) 0.80 Cu2"(aq) + 2e → Cu(s) 0.34 a. As written, is the Keg of the reaction shown above greater than 1 or less than 17 (Select] b. Which species is the reducing agent? [Select ] c. Suppose a voltaic cell was constructed using a Cu and Ag electrode (pictured below). The Cu electrode was placed in a 0.01 M solution of Cu(NO;)2, and the Ag electrode was placed in a 1.00 M solution of AGNO3. What is the Ecell for this voltaic cell? Assume the temperature is 298 K. Also NO; is a spectator ion. ( Select ) Voltmeter Ag Cu sat bridge AgNO= 1.00 M -0.01 M >
Consider the following reaction: O2 (g) + 4H* (aq) + 4FE2* (aq) = 2H20 (1) + 4FE3* (aq) O2 + 4H' + 4e" → 2H2O E° = +1.23 V Fe3+ + e → Fe?+ E° = +0.77 V Calculate the following. E° cell = +2.00 V AG° (in kJ/mol) = [Select ] > >
Given the standard reduction potentials: Zn2*(aq) + 2e- Zn(s) Ag*(aq) + e + Ag(s) E°=-0.76 V E°= 0.80 V Which species is the best oxidizing agent? Ag(s) O Ag*(aq) O Zn(s) O Zn2*(aq)
for the following galvanic elements determine the electromotive force at 25 ° C Cu | Cu2 + 0.01M || Cu2 + | Cu 1.0M Ag | Ag + 0,001M || Cu2 + | Cu 0,01M
Calculate the E° of the following cell: Pt|[Fe(CN)s]*, [Fe(CN)J³l|Cr³*(aq)|Cr Given: EFe(CN)aFe(CN)/4 = 0.36 V; E3 = -0.74 V %3D
Consider the following two half-reactions and their standard reduction potentials. N2(g) +H,0(1) E° = 1.766 V MnO, (s) + 2H,0(1) E° = 1.673 V N,0(g) + 2H*(aq) + 2e¯ → MnO,(aq) + 4H*(aq)+3e¯ 1st attempt l See Calculate E°for the spontaneous redox reaction that occurs when these two half-reactions are coupled. V
Based on the following half-reactions, which is the strongest oxidizing agent? Half-Reaction Ag*(eg) + e-→ Ag(9) Sntag) + 2e -Sn2*ceg) Fe2*(ag) + 2e- → Fe(s) Lit(ag) + e- - E (V) E = 0.80 V E° = 0.15 V E° = -0.45 V E° = -3.04 V - Lics) A. Ag*iag) B. Agis) C. Li*teg) D. Sntteg)
2+ 4+ a. Will Fe+ oxidize Sn to Sn*t ? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Fes+ +e → Fe2+ +0.77 Sn n4+ + 2e → Sn²+ +0.15 O yes O no b. Will dichromate ions oxidize chloride ions to free chlorine in acidic solution? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction e° (V) Cr2 0, + 14H+ + 6e¯ → 2Cr³+ + 7H2O +1.33 Cl2 + 2e → 2C1 +1.36 O yes O no
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.