Question

For the cell shown, the measured cell potential, $E_{cell}$, is -0.3645 V at 25 °C. Pt(s) | H₂(g, 0.893 atm) | H+(aq,? M) || Cd² +(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, $E^0$, are $2H^+(aq) + 2e^- \to H_2(g)$ $E^0 = 0.00 V$ $Cd^{2+}(aq) + 2e^- \to Cd(s)$ $E^0 = -0.403 V$ Calculate the H+ concentration. [H+] = __ M

Name: for the cell shown the measured cell potential ecell is 03645 v at 25 c pts h2g 0893 atm haq m cd2 aq 100 m cds the balanced reduction half reactions for the cell and their respective stand 07492
Uploaded: 2023-08-23T08:12:16-08:00
Duration: 4 min 34 s
Channel: Sri K
Description: for the cell shown the measured cell potential ecell is 03645 v at 25 c pts h2g 0893 atm haq m cd2 aq 100 m cds the balanced reduction half reactions for the cell and their respective stand 07492

          For the cell shown, the measured cell potential, $E_{cell}$, is -0.3645 V at 25 °C.
Pt(s) | H₂(g, 0.893 atm) | H+(aq,? M) || Cd² +(aq, 1.00 M) | Cd(s)
The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, $E^0$, are
$2H^+(aq) + 2e^- \to H_2(g)$  $E^0 = 0.00 V$
$Cd^{2+}(aq) + 2e^- \to Cd(s)$  $E^0 = -0.403 V$
Calculate the H+ concentration.
[H+] = __ M

for the cell shown the measured cell potential ecell is 03645 v at 25 c pts h2g 0893 atm haq m cd2 aq 100 m cds the balanced reduction half reactions for the cell and their respective stand 07492

Added by Steven B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

08/23/2023

Step 1

893 atm) | H+(aq,? M) || Cd² +(aq, 1.00 M) | Cd(s) The half-reactions are: Anode (oxidation): $H_2(g) \to 2H^+(aq) + 2e^-$ $E^0 = 0.00 V$ Cathode (reduction): $Cd^{2+}(aq) + 2e^- \to Cd(s)$ $E^0 = -0.403 V$ The overall cell reaction is: $H_2(g) + Cd^{2+}(aq) Show more…

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For the cell shown, the measured cell potential, $E_{cell}$, is -0.3645 V at 25 °C. Pt(s) | H₂(g, 0.893 atm) | H+(aq,? M) || Cd² +(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, $E^0$, are $2H^+(aq) + 2e^- \to H_2(g)$ $E^0 = 0.00 V$ $Cd^{2+}(aq) + 2e^- \to Cd(s)$ $E^0 = -0.403 V$ Calculate the H+ concentration. [H+] = __ M