What is the pH in the cathode for the following galvanic cell made from the following two half reactions? The initial concentration of gold ion is 3.5x103 M, the initial concentration of permanganate is 6.07 M, and the Ecell is 0.15 V. Assume the temperature is 298K. Au3+ (aq) +3e-→ Aus) E° = 1.52 V MnO4 (aq) + 4H*(aq) 3e-→ MnO2(s) + 2H₂O E = 1.70 V Read more about this topic

What is the pH in the cathode for the following galvanic cell made from the following two half reactions? The initial concentration of gold ion is 3.5x103 M, the initial concentration of permanganate is 6.07 M, and the Ecell is 0.15 V. Assume the temperature is 298K. Au3+ (aq) +3e-→ Aus) E° = 1.52 V MnO4 (aq) + 4H*(aq) 3e-→ MnO2(s) + 2H₂O E = 1.70 V Read more about this topic

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

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 3 Cl2(g) + 2 Fe(s) 6 CI (aq) + 2 Fe3+(aq) Cl2(g) +2 e → 2 Cl-(aq) E° = 1.36 V Fe3+(aq) + 3 e- Fe(s) E° = -0.036 V
a) b) Draw a diagram showing the following electrochemical cell. Label the anode, cathode, reduction half reaction, oxidation half reaction and direction of electron and ion movement. Include an ammonium nitrate salt bridge. Zn(s) 1 M Zn(NO3)2 || 1.M CUNO3 Cu(s) What is the standard cell potential (E°) of this cell?
A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M Ni2+(aq) solution, and another composed of a silver cathode in a 0.10 M Ag+(aq) solution. The Ecell at 20.0oC is measured as +1.03 V. Determine the number of moles of electrons being exchanged in the resulting redox reaction. Select one: a. 1 mol of electrons b. 4 mol of electrons c. 5 mol of electrons d. 2 mol of electrons e. 3 mol of electrons
Could you please solve the last two questions from the second picture?
Consider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Delete
For the galvanic (voltaic) cell 2+ - Fe(s) + Mn²+ (aq) → Fe²+ (aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²+] if [Mn²+] = 0.090 M and E = 0.78 V? Assume T is 298 K 1 4 7 +/- 2 LO 5 8 0.196 M 3 6 9 O X C x 100
The (fictional) metal unobtanium, Ub, has E° = −0.61 V for the reaction: Ub2+(aq) + 2 e− → Ub(s) a) If the galvanic cell shown below is spontaneous, which metal would be oxidized, and which would be reduced? How do you know? Support your answer with the half-reactions and E°cell. b) Write the overall reaction for this galvanic cell in cell notation.
A galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? A. Cu(s) → Cu2+(aq) + 2e- B. Cu2+(aq) + 2e- → Cu(s) C. Ag+(aq) + e- → Ag(s) D. Ag(s) → Ag+(aq) + e- E. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) DOnt need work shown just answer asap Predict the sign of ΔSorxn (positive or negative) for the following reactions: CH3OH(l) → CH3OH(s) CH4(g) + H2O(g) → CO(g) + 3…
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
3. The oxidation of methanol, as described by the equation below, has a AG value of -937.9 kJ/mol. What is the standard cell potential for a methanol fuel cell? 2CH3OH +30₂ → 2CO₂ + 4H₂O