A voltaic cell consists of two Ag/Ag half-cells. In half-cell A, the electrolyte is 0.07 MAgNO3;...
A voltaic cell consists of two Ag/Ag+ half-cells. In half-cell A, the electrolyte is 0.077 M AgNO3; in half-cell B, it is 5.1 x10-4 M AgNO3. What is Ecell at 298.15 K? (enter to 4 decimal places)
In a test of a new reference electrode, a chemist constructs a
voltaic cell consisting of a Zn/Zn2+ half-cell and an
H2/H+ half-cell under the following
conditions: [Zn2+ ] = 0.021 M [H+ ]= 1.3 M
partial pressure of H2 = 0.32 atm. Calculate
Ecell at 298 K (enter to 3 decimal places).
Zn2+ (aq) + 2e −
⟶ Zn(s) E° = − 0.76 V
2H+ (aq) + 2e −
⟶ H2(g) E° = 0.00 V
We were unable...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a cobalt electrode immersed in 1.00 M Co(NO3)2 solution. Cobalt plates out on the cobalt electrode as the voltaic cell runs. The beginning voltage of the cell is +0.467 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is −0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
A voltaic cell consists of an Mn/Mn2+ half-cell and a Pb/Pb2+ half-cell. Calculate [Pb2+] when [Mn2+] is 2.5 M and Ecell = 0.23 V.
Chem 103A Electrochemistry 11. A voltaic cell consists of Ni/Ni" and Co/Co2 half-cells with the following concentrations: IN 0.80 M, [Co] -0.20 M. Assume the temperature is 25*C, Given: Ni/Nit has a standard reduction potential of -0.23 V and Co/Co2 has a standard reduction potential of -0.28 V a) What is the initial Ecell? (You first must decide which way to combine the two half-cells in order to get a spontaneous reaction, i.e., which should be the oxidation reaction and...
A voltaic cell consists of an Mn/Mn2+ half-cell and a Pb/Pb2+ half-cell. Calculate [Pb2+] when [Mn2+] is 2.1 M and Ecell = 0.35 V. _____M
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 is the initial cell potential? Hint: the standard potential of Pb2+ + 2e → Pb(s) is -0.130 and the standard potential of Cu2+ + 2e → Cu(s) is +0.340. Hint #2: Use [Cu2+] as the product and [Pb2+] as the reactant. Ecell = 0.044 Ecell = 0.383 Ecell = 0.426 Ecell...
Question 8 0.5 pts 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 is the initial cell potential? Hint: the standard potential of Pb2*+2e » Pb(s) is -0.130 and the standard potential of Cu2 + 2e -» Cu(s) is +0.340. Hint #2: Use [Cu2*] as the product and [Pb2'] as the reactant. Ecell 0.044 Ecell 0.383 Ecell 0.426 Ecell...
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a nickel electrode immersed in 1.00 M NI(NO3)2 solution. Nickel plates out on the nickel electrode as the voltaic cell runs. The beginning voltage of the cell is +0.487 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is -0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Cd2+} when {Al3+} = 0.306 M and Ecell = 1.27 V. Use reduction potential values of Al3+ = -1.66 V and for Cd2+ = -0.40 V.