3.128 Heating 2.40 g of the oxide of metal X (molar mass ofX = 55.9 g/mol) in carbon monoxide (CO) yields thepure metal and carbon dioxide. The mass of the metalproduct is 1.68 g. From the data given, show that thesimplest formula of the oxide is X2O3 and write abalanced equation for the reaction.
3.128 Heating 2.40 g of the oxide of metal X (molar mass ofX = 55.9 g/mol) in carbon monoxide (CO) yields thepure metal and carbon dioxide. The mass of the metalproduct is 1.68 g. From the data given, show that thesimplest formula of the oxide is X2O3 and write abalanced equation for the reaction.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter11: Stoichiometry
Section: Chapter Questions
Problem 109A: When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of...
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3.128 Heating 2.40 g of the oxide of metal X (molar mass of
X = 55.9 g/mol) in carbon monoxide (CO) yields the
pure metal and carbon dioxide. The mass of the metal
product is 1.68 g. From the data given, show that the
simplest formula of the oxide is X2O3 and write a
balanced equation for the reaction.
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