Which of the following statements is TRUE? Select one: O a. The standard hydrogen electrode uses H2(g, 1 bar) and H*(aq, 0.1 M) O b. The standard hydrogen electrode oxidises a Pt electrode in an aqueous acidic solution Oc. The standard hydrogen electrode reduces a Pt electrode in an aqueous acidic solution O d. The standard hydrogen electrode can only be used to produce H2(g) from H*(aq). The reverse reaction is not possible O e. The potential of the standard hydrogen electrode is always zero

Which of the following statements is TRUE? Select one: O a. The standard hydrogen electrode uses H2(g, 1 bar) and H(aq, 0.1 M) O b. The standard hydrogen electrode oxidises a Pt electrode in an aqueous acidic solution Oc. The standard hydrogen electrode reduces a Pt electrode in an aqueous acidic solution O d. The standard hydrogen electrode can only be used to produce H2(g) from H(aq). The reverse reaction is not possible O e. The potential of the standard hydrogen electrode is always zero

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

An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode Based on the reactions below, which is the stongest reducing agent? +1.22 V MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2- (aq) -0.95 V SnO2(s) + 2H2O() + 4e-→ Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- → Cr(s) + 3OH-(aq) a.Hg2SO4 b.Mn02 c.Cr d.Sn e.Hg Identify the strongest oxidizing agent from the following half-reactions. The standard reduction potentials are listed. +1.22 V Mn02(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H20(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2-(aq) -0.95 V SnO2 (s) + 2H2O() + 4e- Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- Cr(s) + 3OH- (aq) a. MnO2 b.Hg2SO4 c.Sn d.Hg e.Cr
Name: NetID: 21. Electrolysis can be a convenient way to remove a metal from a solution of multiple ions. What mass of aluminum metal (26.982 g mol-¹) can be isolated from a solution of Al2O3 using a current of 125 A over a 12 hour period? A: 503.3
A galvanic cell consist of Mg anode in a 1.0 M Mg(NO3)2 and Al cathode in a 1.0 M Al(NO3)3 solution with NaCl as the electrolyte in the salt solution. a. calculate the electrical energy b. free energy change (G) c. Equilibrium constant (K)
A cell utilizes the following reaction and operates at 298 K: 2H+(aq) + Zn(s) → Zn2+(aq) + H2(g) a.What is the emf of this cell under standard conditions? (Look up E° values). b. What is the emf of this cell when [Zn2+] = 0.050 M, PH2 = 0.25 atm, and the pH = 4.00.(Use pH toget [H+]
Which statements is/are true? a. At the start of the electrochemical reaction, the cell potential (Ecell) of a concentration cell is always zero. b. If 25 mmol of Gd metal forms after electrolysis of Gd ions using a current of 1.0 A for 2 h, the Gd source has a charge of +3.
Please show the step by step solution!
3. Calculate the free energy, AG°, for each electrochemical cell given the following information and determine if the reaction is spontaneous or nonspontaneous. T= 298 K a. E cell =+ 2.10 V, n= 2 b. Каg— 2.2 х 10-3 c. E cell =- 0.677 V, n = 3 =
4. How many grams of copper will be produced if a current of 25 A is passed through CUSO4 solution for 30.0 minutes?
Zn(s) + 2 H*(aq) → Zn²*(aq) + H2(g) 1. What is the effect on the cell potential of a voltaic cell wi h the above reaction when: The pressure of H2 gas is increased in the cathode. c. Sodium hydroxide is added to the cathode half-cell decreasing the [H"]. а. b. Zinc nitrate is added to the anode d. The surface area of the anode is doubled. half-cell.
6. Electrolysis of water using platinum electrode produces oxygen gas at the anode and hydrogen gas at the cathode according to the following half-cell reactions. Anode: 2H20 → 02 + 4H* + 4e Cathode: 4H20 + 4e → 2H2 + 40H- Determine the mass of hydrogen gas that are liberated after 5mins wit a current of 0.2 A. Given atomic mass of hydrogen, H is 1 g/mol, 1 Faraday = 96500 C/mol e
2. A solution at 25 °C contains 1 M Cu2t and 0.010 M Ag*. Which metal will be plated on the cathode first when this solution is electrolyzed? (Hint: Use the Nernst equation to calculate E for each half reaction)