### Electrochemical Cell and Calculating Hydrogen Ion ConcentrationFor the cell shown, the measured cell potential, $E_{\text{cell}}$, is $-0.3657 \text{ V}$ at $25 \degree \text{C}$.**Cell Notation:**\[ \text{Pt(s)} \mid \text{H}_2(\text{g}, 0.777 \, \text{atm}) \mid \text{H}^+(\text{aq}, \, ? \, \text{M}) \parallel \text{Cd}^{2+}(\text{aq}, 1.00 \, \text{M}) \mid \text{Cd(s)} \]**Balanced Reduction Half-Reactions:**\[ 2\text{H}^+ (\text{aq}) + 2\text{e}^- \rightarrow \text{H}_2 (\text{g}) \qquad E^\circ = 0.00 \, \text{V} \]\[ \text{Cd}^{2+} (\text{aq}) + 2\text{e}^- \rightarrow \text{Cd(s)} \qquad E^\circ = -0.403 \, \text{V} \]**Problem Statement:**Calculate the $\text{H}^+$ concentration.**Initial Answer Provided:**\[ [\text{H}^+] = 0.23 \, \text{M} \]**Feedback:**Incorrect#### Explanation:Given the cell potential and standard reduction potentials, you may use the Nernst equation to find the concentration of $\text{H}^+$. The answer provided was found to be incorrect, indicating a need for re-evaluation of the calculation process. Further steps involve adjusting calculations for accuracy.

Ecell = 0.3657 V PH2 = 0.777 atm The balanced reduction half reactions 2 H+ (aq) + 2 e- ----->…

For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777 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, Eº, are 2 H+ (aq) + 2 e- H₂(g) Eº = 0.00 V Cd²+ (aq) + 2 e Cd(s) E° -0.403 V Calculate the H+ concentration. 0.23 [H+] = Incorrect M

For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777 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, Eº, are 2 H+ (aq) + 2 e- H₂(g) Eº = 0.00 V Cd²+ (aq) + 2 e Cd(s) E° -0.403 V Calculate the H+ concentration. 0.23 [H+] = Incorrect M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate Ecell for the following electrochemical cell at 25 °CPt(s) | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Sn2+(aq, 0.350 M), Sn4+(aq, 0.020 M) | Pt(s)The standard reduction potentials are as follows: Sn4+(aq) + 2 e– → Sn2+(s) E° = +0.15 V 2 H+(aq) + 2 e– → H2(g) E° = 0.00 V
For the cell shown, the measured cell potential, Ecell, is –0.3521 V at 25 °C. Pt(s) | H,(g, 0.785 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°, are 2H* (aq) + 2e- - H, (g) E° = 0.00 V Cd²* (aq) + 2e" - Cd(s) E° = -0.403 V Calculate the H* concentration. [H*] = M
Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.38 V; Zn2+ (aq) Zn(s): -0.78 V; Ni2+ (aq) |Ni (s): -0.29 V; Cu2+ (aq)| Cu(s): 0.30 V. Calculate the standard cell potential in V for the cell reaction Cu²+ (aq) + Cd(s)→Cd²+ (aq) + Cu(s) Report your answer with 2 places past the decimal point. Do not put unit in your answer. Type your answer...
edit: Calculate the cell potential for the following galvanic cell at 25°C: Al(s) Al3+ (0.0632 M)|| Au3+ (0.255 M)|Au(s)
For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 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°, are 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7
Pt(s) | H,(g, 0.703 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, Eº, are 2 H¹ (aq) + 2e H₂(g) Cd²+ (aq) + 2 e¯ → Cd(s) D Calculate the H concentration. [H+] = Eº = 0.00 V Eº = -0.403 V M
Two half-reactions are shown with their standard cell potentials. If a galvanic cell is constructed using them, which electrode would be the anode, and what would the cell potential be? Cd2* (aq) + 2e – Cd(s); E=-0.40 V Cr3+ (aq) + 3e → Cr(s); E=-0.74 V Oa. Cadmium, -0.34 V Ob. None of the other options Oc. Cadmium, -1.14 V Od. Chromium, -1.14 V Oe. Chromium, 0.34 V
Calculate the reaction temperature of the electrochemical cell described below which measures a potential of 0.313 V. Cu(s) | Cu2+ (0.80 M) || O2(g) (0.98 atm) | H+ (0.047 M), H2O2 (0.92 M) | Pt(s) (Use R = 8.314 J/mol-K; F = 96485 C/mol)
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 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°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh
Construct a galvanic cell from MnO4- (aq)/MnO2 (s) and H2 O2 (aq)/H2 O (l).a) Write a balanced equation for the cell.b) What is the value of E°cell? standard Ni (s) | Ni2+ (aq) || Ag+ (aq) | Ag (s) is constructed and the standard cell potential is1.03 V.a) Write a balanced reaction for the cell.b) What is ∆G° for the cell?
Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = V
For the cell shown, the measured cell potential E cell -0.365; V at 25 degrees * C . Pr(s)|H 2 (g,0.803 am)|H^ + (aq,?M)||Cd^ 2+ (aq,1.00 M)|Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values E ^ o are 2H^ + (aq)+2e^ - longrightarrow H 2 (g) E ^ o = 0.00V Cd^ 2+ (aq)+2e^ - longrightarrow Cd(s) E ^ o= - 0.403V Calculate the H^ + concentration.