Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M):2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq)a.Write the cell diagram.b. What will be the Eᵒcell? Show solution (use provided SRP table values). Increasing strength as oxidizing agentTable of Standard Reduction PotentialsHalf-ReactionF₂(g) + 2e2F (aq)03(g) + 2H+ (aq) + 2e¯ →→ O₂(g) + H₂OCo³+ (aq) + e-Co²+ (aq)H₂O₂(aq) + 2H(aq) + 2e¯→→→→→→ 2H₂OPbO₂ (s) + 4H+ (aq) + SO (aq) + 2e+ (aq) + e Ce³+ (aq)Ce4+MnO4 (aq) + 8H*(aq) + 5e¯ →→Mn²+ (aq) + 4H₂OAu³+ (aq) + 3e →→→ Au(s)2Cr³+ (aq) + 7H₂OMn²+ (aq) + 2H₂OCl₂(g) + 2e →→→ 2Cl¯ (aq)Cr₂O (aq) + 14H+ (aq) + 6e¯MnO₂ (s) + 4H+ (aq) + 2e¯→→O₂(g) + 4H(aq) + 4e¯ →Br₂(1) + 2e2Br (aq)NO3(aq) + 4H+ (aq) + 3e2Hg²+ (aq) + 2eNO(g) + 2H₂OHg₂+ (aq)Hg2+ (aq) + 2e →→→ 2Hg(1)Ag+ (aq) + e Ag(s)Fe³+ (aq) + e→→→→→→ Fe²+ (aq)O₂(g) + 2H+ (aq) + 2e →H₂O₂(aq)MnO₂ (s) + 4OH(aq)MnO4 (aq) + 2H₂O + 3e¯1₂(s) + 2e21 (aq)O₂(g) + 2H₂O + 4e4OH(aq)Cu²+ (aq) + 2eCu(s)AgCl(s) + eAg(s) + Cl(aq)SO (aq) + 4H+ (aq) + 2e →→→ SO₂(g) + 2H₂OCu²+ (aq) + eCu* (aq)Sn4+4+ (aq) + 2e¯Sn²+ (aq)H₂(g)2H*(aq) + 2ePb²+ (aq) + 2ePb(s)2+Sn²+ (aq) + 2eSn(s)Ni(s)Ni²+ (aq) + 2eCo²+→Co(s)(aq) + 2e¯PbSO4(s) + 2ePb(s) + SO² (aq)Cd(s)Cd²+ (aq) + 2eFe²+ (aq) + 2e→Fe(s)Cr³+ (aq) + 3e→ Cr(s)Zn²+(aq) + 2e¯¯→→→→→→ Zn(s)2H₂O + 2e →→→ H₂(g) + 2OH(aq)Mn²+ (aq) + 2e→ Mn(s)Al³+ (aq) + 3eAl(s)Be(s)→ Mg(s)Be²+ (aq) + 2eMg²+ (aq) + 2eNa (aq) + eCa²+ (aq) + 2eNa(s)Ca(s)Sr2²+ (aq) + 2eSr(s)2+Ba²+ (aq) + 2e →→→ Ba(s)K+ (aq) + e → K(s)Li (aq) +eLi(s)2H₂OPbSO4(s) + 2H₂OE° (V)+2.87+2.07+1.82+1.77+1.70+1.61+1.51+1.50+1.36+1.33+1.23+1.23+1.07+0.96+0.92+0.85+0.80+0.77+0.68+0.59+0.53+0.40+0.34+0.22+0.20+0.15+0.130.00-0.13-0.14-0.25-0.28-0.31-0.40-0.44-0.74-0.76-0.83-1.18-1.66-1.85-2.37-2.71-2.87-2.89-2.90-2.93-3.05Increasing strength as reducing agent

In the cell diagram anode is written on the right side and the cathode is on the left side. At…

Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): 2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq) a. Write the cell diagram. b. What will be the Eᵒcell? Show solution (use provided SRP table values).

Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): 2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq) a. Write the cell diagram. b. What will be the Eᵒcell? Show solution (use provided SRP table values).

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

Similar questions

The voltaic cell Ca(e)]Ca** (ag) || Ni²* (1.0 M)|Ni(s) has a cell potential of 0.290 V at 25°C. What is the concentration of cadmium ion? (Eal = 0.170 V.) Concentration = M
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + Enter the reaction that takes place at the cathode. Include state symbols: + In the external circuit, electrons migrate v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to
Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.
A galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? A. Cu(s) → Cu2+(aq) + 2e- B. Cu2+(aq) + 2e- → Cu(s) C. Ag+(aq) + e- → Ag(s) D. Ag(s) → Ag+(aq) + e- E. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) DOnt need work shown just answer asap Predict the sign of ΔSorxn (positive or negative) for the following reactions: CH3OH(l) → CH3OH(s) CH4(g) + H2O(g) → CO(g) + 3…
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
5) Determine the cell potential for an electrochemical cell based on the following two half- reactions. Be sure to balance the equations to determine the moles of electrons. a. Ca(s) + Cu (ag)-> Ca (ag) + Cu(s) [Ca] = 0.625 M, [Cu] = 0.0150 M b. Na(s) + Pb*(ag) -> Na* (ag) + Pb(s) [Na] = 0.00225 M, [Pb] = 0.825 M c. Cr*(ag) + Cu*(ag)-> Cu(s) + Cr*(ag) [Cr*]=1.85 M, [Cr] = 0.150 M, (Cu] = 0.175 M
A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: Cr(s) + 3 Ag*(aq) → Cr³*(aq) + 3 Ag(s) Which of the multiple choices correctly describes how the cell emf changes when a change is made to the cell? Ca) Adding water to the anode compartment makes the cell emf less positive. C b) Increasing the size of the silver electrode makes the cell emf stay the same. C C) Adding a solution of 1.0 M AGNO, to the cathode compartment makes the cell emf more negative. C d) Adding Na,s to the anode compartment to precipitate chromium sulfide makes the cell emf less positive. Ce) Adding a solution of 5 M Ag* to the cathode compartment makes the cell emf stay the same.
5. Consider the following under acidic conditions: Cu(s) + MnO4¹ (aq) → Mn²+ + Cu²+ i ii Write the balanced half-reaction for the oxidation that occurs. Write the balanced half-reaction for the reduction that occurs. iii Write the balanced redox reaction. iv Write the potential for each half-reaction next to it (the values are in your text) V Calculate the cell potential. vi Calculate AG at 25 °C. vii Is this reaction spontaneous? Why? viii Draw and label the cell for this reaction. ix Write the line notation for the cell.
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O