A student has 3.86 g of iron metal how many moles of iron does the student have? Given your answer and the fact that rust has the formula Fe2O3 how many miles of oxygen would be required to convert all of the iron to rust?

A student has 3.86 g of iron metal how many moles of iron does the student have? Given your answer and the fact that rust has the formula Fe2O3 how many miles of oxygen would be required to convert all of the iron to rust?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 84QAP: Suppose that the atomic mass of C-12 is taken to be 5.000 amu and that a mole is defined as the...

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