Part A Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag*(aq) +e¯ → Ag(s) What mass of silver plates onto the cathode when a current of 6.1 A flows through the cell for 79 min ? Express the mass in grams to two significant figures. ΑΣφ g. — ш Submit Request Answer Provide Feedback

Part A Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag*(aq) +e¯ → Ag(s) What mass of silver plates onto the cathode when a current of 6.1 A flows through the cell for 79 min ? Express the mass in grams to two significant figures. ΑΣφ g. — ш Submit Request Answer Provide Feedback

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

How many minutes does 8.208 A of current need to be applied to plate 1.402 g of aluminum onto a substance according to the following half reaction? AI3+ (аg) + 3 е > Al(s) Your Answer: Answer units
A current of 7.83×104 A is passed through an electrolysis cell containing molten KCI for 20.7 days. (a) How many grams of potassium are produced? 6.0 Submit Answer g (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L
Tech Please don't provide the handwriting solution
Can you please answer these two sub problems and show all of the steps to the solution
Need answer step by step
Balance the following reaction, determine the reducing and oxidizing agent, the half reaction at the cathode and anode, drawn the line notation and calculate the cell potential.
Consider the electrolysis reactions cathode Cu²+ (aq, 0.125 M) + 2e anode H₂O(1) = whose standard reduction potentials can be found in this table. Calculate the voltage needed to drive the net reaction if the current is negligible. Ecell = Cu(s) 10₂(g, 1 bar) + 2 H+ (aq, 0.243 M) + 2€¯ The cell has a resistance of 63.0 and a current of 7.26 mA when the cathode overpotential is 0.223 V and the anode overpotential is 0.084 V. Calculate the voltage needed to overcome these effects and drive the net reaction. Ecell = V V
Decide whether or not each metal dissolves in 1 mol L-1 HIO3(aq). Standard Electrode Potentials at 25 °C Reduction Half-Reaction E° (V) Au3+ (aq) +3e → Au(s) 1.50 IO3 (aq)+6H+(aq) + 5e7 →12 (s) + 3H2O(1) 1.20 Ni²+(aq) + 2e → Ni(s) -0.23
4
Question 6 ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate 0.063 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 14 minutes at a current of 2.3 A given the following reaction. Z3+(aq) + 3e- → Z(s) Atomic Mass: Z: 176.56 g/mol Round your answer to 2 decimal places.
Part A Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag (aq) + e¯→ Ag(s) What mass of silver would plate onto the cathode if a current of 8.1 A flowed through the cell for 63 min ? Express your answer to two significant figures and include the appropriate units. Templates Symbols uado redo resat keyboard shortcuts help, Value Units m =