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A metal forms the fluoride MF3. Electrolysis of the molten fluoride by a current of 3.86 A for 16.2 minutes deposits 0.660 g of the metal. Part A Calculate the molar mass of the metal.

A metal forms the fluoride MF3. Electrolysis of the molten fluoride by a current of 3.86 A for 16.2 minutes deposits 0.660 g of the metal. Part A Calculate the molar mass of the metal.

Chemistry
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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Can someone please help with question 6

1302 - 4.3 - Exercise 18.124 - Copy - Copy 6 of 15 I Review I Constants | Periodic Table A metal forms the fluoride MF3. Electrolysis of the molten fluoride by a current of 3.86 A for 16.2 minutes deposits 0.660 g of the metal. Part A Calculate the molar mass of the metal. ? M = 8.49 g/mol Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Transcribed Image Text:1302 - 4.3 - Exercise 18.124 - Copy - Copy 6 of 15 I Review I Constants | Periodic Table A metal forms the fluoride MF3. Electrolysis of the molten fluoride by a current of 3.86 A for 16.2 minutes deposits 0.660 g of the metal. Part A Calculate the molar mass of the metal. ? M = 8.49 g/mol Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
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