Choose which direction is spontaneous for the following reaction.  Calculate Eo for the spontaneous reaction.  If you now calculate E using the Nernst equation, you find that E = 1.18 eV.  Calculate the concentration of Al3+ if the concentration of Fe2+ is 2.25M. If you let this battery run at 3.6 amps, how long in minutes would you have to wait to lose 1.3 grams of your anode?   Fe2+  +  Alo  <--->  Feo  +  Al3+

Q: What is the equilibrium constant (K) at 25°C for the following cell reaction? Sn(s) + Pb²+ (aq) →…

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Q: Given the following battery: Au+1/Au0 and Ni+2/Ni0 calculate EO. If you wanted to improve your…

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Q: 1. For the following electrochemical cell at 25°C: Fe(s) Fe (aq) ||H(aq) | Pt, H₂(g) (P=1.00 atm) a.…

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Q: 33. Calculate the copper(II) ion concentration at 25 °C in the cell Zn(s) + Cu²*(aq) → Zn²"(aq, 1.0…

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Q: Calculate Eo, ΔG0 and K for a battery of Fe+2/ Fe0 and Al+3/ Al0.  If you want to hurt the battery…

A: Given Battery: Fe+2/ Fe0 and Al+3/ Al0To determine:1) Eo, ΔG0 and K2) Concentration of Al3+ if the…

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Q: n electrochemical cell has an iron electrode in a solution of Fe2+ ions on one side, and a nickel…

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Q: 5. Consider the following galvanic cell at 298 K. B(s) | B*(0.0050 M) || A²*(0.0100 M)| (s) A2+(aq)…

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Q: The following reaction occurs at 298 K:  Zn (s) + 2 Ag+ (aq) ---> Zn2+ (aq) + 2 Ag (s) i. Sketch a…

A: E°cell= E°cathode- E°anode  G°=-nFE°  G°= RT In K

Q: Use the tabulated half-cell potentials in table 18.1 to calculate the equilibrium constant (K) for…

A: Recall the given reaction         2Als + 3 Mg2+aq → 2Al3+aq + 3MgsWrite the cell…

Q: If 15.00 A of current is applied, how long would it take to produce 25.0 g of Cr(s)? hr

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Q: Eº Ni²+ + 2e → Ni Zn²+ +2e → Zn - 0.76V Zn(s) + Ni²+ (aq) Zn²+ (aq) + Ni(s) This reaction runs a…

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Q: Consider the following reaction at 298 K. Ni²+ (aq) + Cd(s) → Ni(s) + Cd²+ (aq) Which of the…

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A: The balanced reaction taking place is is, =&gt; 3 Fe2+ (aq) + Cr3+ (aq) -------&gt; Cr (s) + 3 Fe3+…

Q: Given the following battery:  Au+1/Au0 and Ni+2/Ni0 calculate EO.  If you wanted to improve your…

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Q: Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of…

A: Given-&gt; [Be2+] = 0.793 V [V2+] = 2.01 V

Q: Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question.  Which…

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Q: 3. For the cell notations in the previous problem, write the corresponding balanced reactions. .…

A: Galvanic cell reaction:-  2Cr(s) + 3Cu+2(aq) --------&gt; 2Cr+3(aq) + 3Cu(s) Anode is the place…

Q: Consider a voltaic cell consisting of a magnesium electrode in contact with 1.0 M Mg(NO3)2 and a…

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Q: For the questions of Exp 20 Electrochemistry, Part A: Determination of the Faraday Constant Table 1:…

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Q: MISSED THIS? Read Section 20.4 (Pages 903-913); Watch KCY 20.4 Decide whether or not each of the…

A: EoCu2+/Cu = 0.34 V EoAu3+/Au = 1.50 V EoNO3-/NO = 0.96 V   Above values decide feasibility of…

Q: For the questions of Exp 20 Electrochemistry, Part B: EMF of Galvanic Cell Table 2: Electromotive…

A: the equilibrium constant (Kp) for the vaporization of bromine at 59.7°C:Bromine Vaporization…

Q: Consider the two half-reactions given below: Mg2+ + 2 e → Mg Ag* + e → Ag E° = -2.37 V E° = 0.80 V…

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Q: Calculate the Eocell for this reaction occurring under standard conditions: 2 H+ (aq)   +   Fe (s)…

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Q: Find K for the following reaction at 25°C. Ecell = 0.45 V Pb2+ + Fe(s) Pb(s) + Fe2+ (aq) 8.6 x 10-6…

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A: Answer :-  A) Mass of Cu metal dissolved = 0.997 g  B) Mass of Ag metal deposited = 3.39 g…