Calculate ℰ for the cell reaction at 298 K with the concentrations given below:   2 Al(s) + 3 Fe2+ (aq, 2.0 M) → 2 Al3+ (aq, 0.03 M) + 3 Fe(s) Al3+ + 3e- → Al   -1.676V Fe2+ + 2e- → Fe   -0.440V Provide your answer rounded to 3 significant figures.

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.18 minutes for a current…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.67 minutes for a current…

A: Mass = 0.07 g Current = 1.89 A Time = 1.67 min = 1.67×60 sec Atomic mass = ?

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Q: Consider a cell reaction at 25oC where n=3.  7. Consider a voltaic cell at 25oC in which the…

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Q: 1. Find ΔG in J for: X5+(aq) + 5e- → X(s) E = -0.56 V 2.  2Al(s) + 6H+(aq) → 2Al3+(aq) + 3H2(g)…

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Q: Part B Calculate the standard cell potential at 25 °C for the reaction where AH = -803 kJ and AS =…

A: ∆G° = ∆H° - T∆S°  T = Temperature ∆G° = - nFE°  n = number of electrons involve  F = 96500 C mol-1…

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Q: Calculate Ecell for the following voltaic cell.     The reaction is spontaneous or not?…

A: Given data: Concentration of Al3+ = 0.26 M Concentration of Sn4+ = 0.086 M Concentration of Sn2+ =…

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Q: 1. Write the reduction half-cell reaction and their corresponding standard reduction potentials (°E)…

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Q: Calculate AG° (in kJ) for the following reaction: 31, (s) + 2Fe(s) →2FE** (aq) +6I¯(aq) 232 O -111 O…

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Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

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Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.42 minutes for a current…

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Q: What is the cell potential for the following reaction at 25 °C?  Ni(s) + Cu2+(0.010 M) →…

A: The cell reaction given is, => Ni(s) + 2 Cu2+(0.010 M) → Ni2+(0.0010 M) + 2 Cu+(1.0 M) Given:…

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

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Q: Calculate Ecell for the following electrochemical concentration cell:   Write your answer with three…

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Q: 17.45. Calculate the E the reaction cell value at 25°C for the cell based on Fe³+ (aq) + Cr2+ (aq) →…

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Q: For the reaction 2Co³+ (aq) + 2Cl(aq)→2Co2+ (aq) + Cl₂(g). E=0.483 V what is the cell potential at…

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A: Given concentrations:[H+] = 0.152 M[NO3- ] = 0.470 M[Fe3+ ] = 0.885 M[NO] = 0.623 MFirst, let's…

Q: onsider a galvanic cell at T = 298K. F = 96 485C. the beginning (to), [Ca²+] = 0.01M, [H*] = 1M,…

A: At cathode-           Ca2+ (aq)  + 2e-      ----->    Ca 0  (s)…

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Q: what is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0140 V and n =…

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A: Electrode potential of the cell (E )

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

A: Cell potential is determined by Nernst equation.

Q: Half-reaction E° (V) I2(s) + 2e→ 21I(aq) 0.535V Pb"(aq) + 2e → Pb(s)|-0.126V Zn-(aq) + 2e →…

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Q: For a cell reaction at 25° C where n= 2 and E° - 0.57 V calculate K. Give your answer as log(k).

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Q: At the beginning (to), [Ca²+] = 0.01M, [H*] = 1M, [Hfo²+] = 2M. Consider the half-reactions below:…

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Q: What is the equilibrium constant K at 25.0 °C for an electrochemical cell when E° = +0.120 V and n =…

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Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0135 V and n =…

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Q: galvanic cell at T = 298K.   F = 96 485C. At the beginning (t0), [Ca2+] = 0.01M, [H+] = 1M, [HfO2+]…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0360 V and n =…

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