14. In a electrochemical cell, metal D can displace Fe?"(aq) but not Mg"(aq). Identify themetal D.D2* (aq) + 2e → D (s)Reduction Half-ReactionVE°red-1.663+Al (aq) + 3e¯ -→ Al (s)24+Са (ag) + 2е -> Са (s)2+Cu (aq) + 2e → Cu (s)-2.87+0.342+-0.44Fe (aq) + 2e → Fe (s)2+-2.37Mg (aq) + 2e Mg (s)2+-0.76Zn (aq) + 2e → Zn (s)A. AlВ. СаС. СиD. Zn

14. In a electrochemical cell, metal D can displace Fe2"(aq) but not Mg (aq). Identify the metal D. D2* (ag) + 2e → D (s) Reduction Half-Reaction V red' -1.66 E° 3+ Al (aq) + 3e Al (s) 2+ Ca (aq) + 2e Ca (s) 2+ Cu (ag) + 2e Cu (s) 24 Fe (aq) + 2e" Fe (s) 2+ -2.87 +0.34 -0.44 -2.37 Mg (aq) + 2e Mg (s) 2+ -0.76 Zn (aq) + 2e Zn (s) A. Al В. Ca Cu D. Zn С.

14. In a electrochemical cell, metal D can displace Fe2"(aq) but not Mg (aq). Identify the metal D. D2* (ag) + 2e → D (s) Reduction Half-Reaction V red' -1.66 E° 3+ Al (aq) + 3e Al (s) 2+ Ca (aq) + 2e Ca (s) 2+ Cu (ag) + 2e Cu (s) 24 Fe (aq) + 2e" Fe (s) 2+ -2.87 +0.34 -0.44 -2.37 Mg (aq) + 2e Mg (s) 2+ -0.76 Zn (aq) + 2e Zn (s) A. Al В. Ca Cu D. Zn С.

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

G ロ・ロ A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ MnO2 (s) + 4H* (aq) +2Cr²* (aq) → Mn²* (aq) + 2H2O (1) +2Cr³+ (aq) Suppose the cell is prepared with 0.190 M H* and 6.41 M Cr²+ in one half-cell and 0.205 M Mn2+ and 1.94 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ ☐ x10 μ
4. Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is K for the following balanced reaction, if E = +0.0218 V? 3Zn+² (aq) + Cr(s) 3Zn(s) + 2Cr³+ (aq) →
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)
A chemist designs a galvanic cell that uses these two half-reactions: 3+ 2+ Fe (aq)+e → Fe (aq) Cro (aq) + 4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is half-reaction spontaneous as written. 0 standard reduction potential Ed=+0.771 V 'red E 'red = -0.13 V ロ→ロ × x10 5
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
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.
At 298 K, what is E (in V) for the electrochemical cell below when [Cd2+] = 4.500 M and [Cu2+] = 0.009 M ? Cd(s) | Cd2+(aq) || Cu2+(aq) | Cu(s) Cu2+ (aq) + 2e– → Cu(s) 0.34 Cd2+ (aq) + 2e– → Cd(s) –0.40
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cu²+ (aq) + Pb(s) → Cu(s) + Pb²+ (aq) 2+ Cu²+ (aq) + 2e Pb²+ (aq) + 2e → Cu(s) Fre 0.337 V → Pb(s) Fe -0.126 V red = Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be | than zero.