For the cell shown, the measured cell potential, \( E_{\text{cell}} \), is \(-0.3621 \, \text{V}\) at \(25^\circ \text{C}\).\[\text{Pt(s) | H}_2\text{(g, 0.853 atm) | H}^+\text{(aq, ? M) || Cd}^{2+}\text{(aq, 1.00 M) | Cd(s)}\]The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, \( E^\circ \), are:\[\begin{align*}2\text{H}^+\text{(aq) + 2e}^- & \rightarrow \text{H}_2\text{(g)} \quad E^\circ = 0.00 \, \text{V} \\\text{Cd}^{2+}\text{(aq) + 2e}^- & \rightarrow \text{Cd(s)} \quad E^\circ = -0.403 \, \text{V}\end{align*}\]Calculate the \(\text{H}^+\) concentration.\[[\text{H}^+] = \boxed{\phantom{0}} \, \text{M}\]

Answered: Image /qna-images/answer/d89c9ad9-1c59-4956-969b-980dcea70df7.jpg

For the cell shown, the measured cell potential, Ecel, 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 2 H* (aq) + 2 e¯ –→ H, (g) E° 0.00 V Cd²+ (aq) + 2 e¯ Cd(s) E° = -0.403 V %3D Calculate the Ht concentration.

For the cell shown, the measured cell potential, Ecel, 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 2 H (aq) + 2 e¯ –→ H, (g) E° 0.00 V Cd²+ (aq) + 2 e¯ Cd(s) E° = -0.403 V %3D Calculate the Ht concentration.

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

[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (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) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M
Calculate ΔG° for the redox reaction represented by the cell diagram Pt(s) | Cl2(g, 1 atm) || ZnCl2(aq, 1 M) | Zn(s).
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
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.
For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 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, ?o, are 2H+(aq)+2e−⟶H2(g) ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s) ?o=−0.403 V Calculate the H+ concentration in M.
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)