Suppose a concentration cell of: Cu(s) | Cu2+(dilute) || Cu2+(concentrated)| Cu(s) is made with the following...
A Cu/Cu2+ concentration cell has a voltage of 0.22 V at 25 ∘C. The concentration of Cu2+ in one of the half-cells is 1.6×10−3 M . What is the concentration of Cu2+ in the other half-cell? (Assume the concentration in the unknown cell to be the lower of the two concentrations.)
A Cu/Cu2+ concentration cell has a voltage of 0.24 V at 25 ∘C. The concentration of Cu2+ in one of the half-cells is 1.6×10−3 M . What is the concentration of Cu2+ in the other half-cell? (Assume the concentration in the unknown cell to be the lower of the two concentrations.) Express your answer using two significant figures.
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial concentrations of Pb2+ and Cu2+ are 0.0530 M and 1.60 M , respectively. 1. What is the initial cell potential? 2. What is the cell potential when the concentration of Cu2+ has fallen to 0.200 M ? 3. What is the concentration of Pb2+ when the cell potential falls to 0.370 V ?
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 oC. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Cu2+(ag) + Pb(s) → Cu(s) + Pb2+(ag) Hint: [Pb2+] + [Cu2+] = (1.5M + 0.05M) = 1.55 M total Hint: the standard potential of Pb2+ + 2e- → Pb(s) is -0.130 and the standard potential...
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial concentrations of Pb2+ and Cu2+ are 5.30×10−2 M and 1.70 M, respectively. Part A- What is the initial cell potential? Express your answer using two significant figures. Part B- What is the cell potential when the concentration of Cu2+ has fallen to 0.230 M ? Express your answer using two significant figures. Part C- What are the concentrations of Pb2+ and Cu2+ when...
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 °C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Cu2+ (aq) + Pb(s) + Cu(s) + Pb2+ (aq) Hint: [Pb2+] + [Cu2+] = (1.5M + 0.05M) = 1.55 M total Hint: the standard potential of Pb2+ + 2e → Pb(s) is -0.130 and the...
Part C. Effect of Concentration on Cell Potentials • Ecall for the Cu(s). Cu2+||Ag*, Ag(s) system: 0.450 V 0,851 v • Ecate for the Cu(s). Cu2+||Ag, Ag(s) system after the addition of 6M NH: • Write the balanced redox reaction for the entire cell: • • How many electrons are transferred? Use the Nernst Equation (given below) to calculate the concentration of Cu left in the solution Een = Ecen (0:0257) in (1960 [Cu2+] =
A Review Constants Periodic Table A Cu/Cu2+ concentration cell has a voltage of 0.22 V at 25°C. The concentration of Cu²+ in one of the half-cells is 1.6x10-3 M. Part A What is the concentration of Cu + in the other half-cell? (Assume the concentration in the unknown cell to be the lower of the two concentrations.) Express your answer using two significant figures. TO ADD A A O O ? Cu2+] = Submit Previous Answers Request Answer
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...
In an electrochemical cell composed of Cu(s)/Cu2+(aq, o.10M)||Cu2+(aq, 1.0M) |Cu(s), Which concentration of Cu would the anode be sitting in? Which concentration of Cu would the cathode be sitting in?