Calculate quantity of materials produced from the electrolysis of a molten salt.A current of 17.3A is passed through an electrolysis cell containing molten MgCl2 for 37.2 minutes.(a) Predict the products of the electrolysis and write the reactions occurring at the anode and cathode. Write electrons as e.Use smallest integer coefficients possible and omit states. If a box is not needed, leave it blank.Cathode reaction:++Anode reaction:++(b) Calculate the grams of metal or liters of gas formed at the cathode and anode (assume gases are at 298 K and 1.00 atm).Formed at cathode:Formed at anode:Өgrams or litersgrams or liters

To predict the products of the electrolysis of molten MgCl2 and write the reactions occurring at the…

Answered: Calculate quantity of materials…

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...

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16-20 Fill in the blanks with the reagents needed: 16 17 18 HO
A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II) sulphate solution. The cathode was made of pure copper. The mass of the cathode before the electrolysis was 0.52 g. After the electrolysis, mass of the cathode was 1.75 g. a. If the current used was 1.5 A, for how many minutes was the electrolysis performed? b. Calculate the magnitude of the current that must be used so that the time of electrolysis can be shortened to 20 minutes.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous ScCl3 solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C Ch(g) + 2 e → 2 Cl'(aq) 1.360 02(g) + 4 H30*(aq) + 4 e» 6 H2O() 1.229 2 H2O(1) + 2 e– H2(g) + 2 OH (aq) -0.828 Sc*(aq) + 3 e - Sc(s) -2.080 Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? V +
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The electrolysis of SnCℓ4 at high temperature produces tin metal. If a constant electricalcurrent of 15.00 × 103 ?? flows for exactly two hours, calculate the number of tin atomspresent in the metal produced during this time.

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