A galvanic cell has an iron electrode in contact with 0.19 MFeSO4 and a copper electrode in contact with a CuSO4 solution. If the measured cell potential at 25 ∘C is 0.60 V, what is the concentration of Cu2+ in the CuSO4 solution? Express your answer using two significant figures. |
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A galvanic cell has an iron electrode in contact with 0.19 MFeSO4 and a copper electrode...
A galvanic cell has an iron electrode in contact with 0.20 M FeSO4 and a copper electrode in contact with a CuSO4 solution. If the measured cell potential at 25 ∘C is 0.55 V , what is the concentration of Cu2+ in the CuSO4 solution? Express your answer using two significant figures.
A galvanic cell has an iron electrode in contact with 0.12 M FeSO4 and a copper electrode in contact with a CuSO4 solution. PartA f the measured cell potential at 25 °C is 0.64 V, what is the concentration of Cu+ in the Cus04 solution? Express your answer using two significant figures. 2+ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Consider a galvanic cell that uses the reaction Cu (s) + 2Fe+ (aq) Cu2+ (aq) + 2Fe+ (aq) Part A What is the potential of a cell at 25 C that has the following ion concentrations? Fel 1 - 1.5x10-4M. Cu2+1 -0.29 M. Fe2+1 -0.18 M Express your answer to two significant figures and include the appropriate units. HA ? Value Units Submit Resvest Answer A galvanie cel has an iron electrode in contact with 0.19 M FeSO, and a...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 9.2×10-5 M? 1 pts Tries 0/8 The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.160 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.) 1 pts...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a) What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 7.5×10-8 M? b) The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.109 V. What is [Cu2+] (in mol/L)? (Assume Cu2+ is reduced.) c) A calibration curve...
Electrochemical Measurement of Concentration An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. What is the potential of this cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 7.1×10-10 M? 1. 0.069 V 1 pts You are correct. 2. The copper electrode of the above cell is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.193 V. What is [Cu2+] (in mol/L)? (Assume...
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5. A galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with CuSO solution. If the measured cell potential at 25°C is 0.67 V, what is the concentration of Cu²+ in the CuSO, solution? [Cu?'] = 8.9 x 10
Be sure to answer all parts. A galvanic cell consists of a silver electrode in contact with 305 mL of 0.100 M AgNO3 solution and a magnesium electrode in contact with 265 mL of 0.700 M Mg(NO3)2 solution. (a) Calculate E for the cell at 25°C. V (b) A current is drawn from the cell until 2.20 g of silver have been deposited at the silver electrode. Calculate E for the cell at this stage of operation. V
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.068 V at 298 K. Based on the cell potential, what is the concentration of Cu2+ in this solution? Express your answer to one significant figure and include the appropriate units.
Answer all question (a-d)
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Consider a galvanic cell which has an Iron electrode submerged in a Fe(NO3)2 soln. and a Gold electrode submerged in a Au(NO3)3 soln. a) Find the Ecell of this cell under standard conditions: (2pts) Ans: Au3+ (aq) + 3e = Aus) ER 1.50 V + 2e = Fe(s) Er = -0.44 V Fe2+ (aq) b) Write out the balanced net reaction of this cell? (3pts) c) What is the cell potential if the concentration...