Water is electrolyzed by passing a current of 0.500 A through 1.00 L of 1.00M Na2SO4 solution for 120 minutes. Determine the pH of the solution in the cathode chamber after the electrolysis was stopped. Assume that the volume of the cathode chamber is 500. mL. You may assume the temperature is 25 °C. 1.428 7.000 1.127 12.572 12.873

Water is electrolyzed by passing a current of 0.500 A through 1.00 L of 1.00M Na2SO4 solution for 120 minutes. Determine the pH of the solution in the cathode chamber after the electrolysis was stopped. Assume that the volume of the cathode chamber is 500. mL. You may assume the temperature is 25 °C. 1.428 7.000 1.127 12.572 12.873

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

Electrolytic process of determining molar mass. An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x 103 s, 8.50 g of elemental X are formed. What is the molar mass of X and at which electrode does X appear?
When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes,the half-reactions are 2I–(aq) → I2(aq) + 2e– 2H2O(l) + 2e– → H2(g) + 2OH–(aq) How many grams of iodine are produced when a current of 8.15 mA flows through thecell for 12.6 min (756 s)?
A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00 x 10–4 M in the two half-cells. The reduction potential of Ni2+ is –0.23 V. Calculate the potential of the cell at 25°C.
Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to measure the amount of electricity passing through a circuit. In this meter, a small, fixed fraction of the total current supplied to a household was passed through an electrolytic cell, plating out zinc at the cathode. Each month the cathode could then be removed and weighed to determine the amount of electricity used. If 0.25% of a household’s electricity passed through such a coulometer and the cathodeincreased in mass by 1.83 g in a month, how many coulombs of electricity were used during that month?
When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PbSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 80.0 A is fed into a car battery for 63.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. x10 0.0 X μ 010 3
The silver zinc battery is used in hearing aids. Explain the fundamental redox reactions that occur in this battery and calculate the theoretical cell potential for this system.
Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode
How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an electrolytic cell, if a current of 15.9 A is passed through an aqueous solution of CuSOa? 19.4 min 32.2 min 24.0 min 33.9 min 26.8 min
The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′ where n is the number of electrons transferred, F is Faraday's constant, 96.5 kJ·mol−1·V−1, and ΔE∘′ is the difference in reduction potential. For each of the given reactions, determine the number of electrons transferred (n) and calculate standard free energy (ΔG∘′) . Consider the half-reactions and overall reaction for reaction 1. half-reactions: fumarate^2− + 2H^+ ↽−−⇀ succinate^2− CoQH2 ↽−−⇀ CoQ + 2H^+ overall reaction: fumarate^2− + CoQH2↽−−⇀succinate^2− + CoQ ΔE∘′= −0.009 V n=____ ΔG∘′= ____ (kJ⋅mol^−1) Consider the half-reactions and overall reaction for reaction 2. half-reactions: cytochrome (c1) (Fe^2+) ↽−−⇀ cytochrome (c1) (Fe^3+) cytochrome (c) (Fe^3+) ↽−−⇀ cytochrome (c) (Fe^2+) overall reaction: cyt (c1) (Fe^2+)+cyt (c) (Fe^3+)↽−−⇀cyt (c1) (Fe^3+)+cyt (c) (Fe^2+) ΔE∘′=0.034 V n= ____ ΔG∘′=____(kJ⋅mol^−1)
Enter your answer in the provided box. A constant current is passed through an electrolytic cell containing molten MgCl₂ for 11.5 h. If 3.40 x 105 g of Cl₂ are obtained, what is the current in amperes? A
Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)