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A concentration cell composed of Cu(s)/Cu2+(aq, 0.10M)||Cu2+(aq, 1.0M)| Cu(s) is connected to a voltmeter. Initially 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?
Please answer asap 1 points A concentration cell composed of Cuscu2ca. 0.101 102 raq, 10ml Cuisisconnected to a voltmeter. Initially a reading of 29.6m was obtained. The cel wing for a few minutes How has the voltage change compared to the initial reading? Why did this change occur?
In the following cell, A is a standard Cu2+Cu electrode connected to a standard hydrogen electrode. If the voltmeter reading is +0.34 V, which half-reaction occurs in the left-hand cell compartment? Given: Standard reduction potential of the H1/H2 and Cu2*/Cu couples are 0.00 and +0.34 V, respectively. Holo H2(g) --> 2H+ (aq) + 2e7 2H(aq) + 2e --> H2(g) Cu(s) --> Cu2(aq) + 2e Cu2(aq) + 2e --> Cu(s)
QUESTION 8 Refer to the data you obtained in the simulation for the concentration cells. Select the correct statements that describe the concentration cell with half cells containing 0.01 M Cu2+ and 0.10 M Cu2+ respectively The voltage is 29.6 mV The voltage is 59.2 mV The solution containing 0.1 M Cu2+ is at the cathode The solution containing 1.0 M Cu2+ is at the cathode The solution containing 0.1 M Cu2+ is at the anode The solution containing 0.01...
Conceptual: Consider a Sn(s)|Sn2+(aq) || Cu2+(aq)|Cu(s) cell. If the Sn2+ concentration is increased, what will happen to the measured Ecell value? • Calculation, full-reaction Nernst equation: Use the full Nernst equation to calculate Ecell for the conditions described… • Easier: Ni | Ni2+(0.300 M) || Cu2+(0.002 M) | Cu • Harder: Al | Al3+(0.002 M) || Cu2+(4.00 M) | Cu • Calculation, half-reaction Nernst equation: Use the Nernst equation to calculate E at pH 3.00 and [Cl- ] = 0.0035...
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady current of 0.0795 A is drawn from the cell as the electrons move from the Cr electrode to the Cu electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? s...
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+] =
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...
A voltaic cell set up utilizing the reaction Cu(s) + 2 Ag+ (aq) → Cu2+ (aq) + 2 Ag (s) has a cell potential of 0.45 V at 298 K. Describe how the potential of the cell will change as the cell is discharged. At what point does the cell potential reach a constant value? Explain your answer
An electrochemical cell is constructed in which a Cut(1.00 M)Cu(s) half-cell is connected to an H30+(aq)H2(1 atm) half-cell with unknown Hz0+ concentration. The measured cell voltage is 0.793 V, and the Cu Cu half-cell is the cathode. What is the pH in the H3O+Hhalf-cell? The standard reduction potential for the Cu Cu half-cell is 0.522 V. pH = Submit Answer Try Another Version 3 item attempts remaining