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: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter4: Reactions In Aqueous Solution
Section: Chapter Questions
Problem 62QAP: Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker...
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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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