Pt1
An electrochemical cell is set up at 25°C based on the overall reaction represented by the balanced equation shown below. The cell initially has [Cr3+] = [Cu2+] and E°cell = +1.08 V. 3Cu2+(aq)+2Cr(s)harpoon_left.pngharpoon_rigth.png3Cu(s)+2Cr3+(aq)
-Using the relationship given in part 1, calculate Ecell if [Cu2+] = 1.453 M and [Cr3+] = 0.00209 M, assuming that the temperature remains at 25°C. Give your answer to two places after the decimal. (R = 8.314 J/mol·K and F = 9.65 × 104 C/mol e–)
Answer :-
Firstly a balanced overall cell reaction is written by writing two halves reaction of half cells and number of electrons transferred. Then Nernst equation is used.
The answer is given in the image,
Pt1 An electrochemical cell is set up at 25°C based on the overall reaction represented by...
An electrochemical cell is set up at 25°C based on the overall reaction represented by the balanced equation shown below. The cell initially has [Cr3+] = [Cu2+] and E°cell = +1.08 V. $$3Cu2+(aq)+2Cr(s)3Cu(s)+2Cr3+(aq) How many moles of electrons are transferred per reaction cycle (i.e., for 1 cycle of the equation as written)? 6 Part 3 (1 point) Using the relationship given in part 1, calculate Ecell if [Cu2+] = 1.453 M and [Cr3+] = 0.00176 M, assuming that the temperature remains...
When the Cu2+ concentration is 6.58×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.979V. What is the Cr3+ concentration? 3Cu2+(aq) + 2Cr(s)3Cu(s) + 2Cr3+(aq) Answer: M When the Cu2+ concentration is 2.71×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 0.971V. What is the Cr3+ concentration? 3Cu2+(aq) + 2Cr(s)3Cu(s) + 2Cr3+(aq) Answer: M
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Consider an electrochemical cell based on the following cell diagram: Pt1 Cut(aq), Cu2+ (aq) || C12(), CI (aq) | Pt Given that the standard cell emf is 1.20V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E*(Cu?+/Cut)? A) 1.01V B) 1.06 V C) 0.16 V D) 2.56 V E) -0.16 V
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0 What is the Ecell for the cell represented by the combination of the following 4) half-reactions? 2Hg2+(aq) + 2e-→Hg22+(aq) Cr3t(ag)+3eCr(s) E-0.92 V B) 1.28 V 9) 0.18 V A) 2.12 V D) 1.66 V E)-0.18 V 5) Examine the following half-reactions and select the weakest oxidizing agent among the 5)_ species listed. E。= 0.854 V E1.185 V K+(aq) + e-→ K(s) F20(aq) + 2H+(aq) + 4e-→ 2p-(aq) + H20() E。= 2.153 V A) F2o(ag) B) AuBr4Taq) C) Mn2+(ag) D)...
A galvanic cell is assembled from one half cell with a nickel electrode immersed in Ni 2+ aqueous solutions in one beaker where [Ni2+] = 1.2 M coupled to a second half cell with a chromium electrode immersed in a Cr3+ aqueous solution to give Ecell = +0.55 V at 25 °C. 3Ni2+(aq) + 2Cr(s) → 3Ni(s) + 2Cr3+(aq) Eϴ cell = +0.50 V Calculate the concentration of the chromium ions [Cr3+] in solution. (A) 1.9 x10^–1 M (B) 6.7...