A student carried out the reaction below starting with 1.993 g of unknown (X2CO3), and found that the mass loss due to CO2 was 0.593 g. X2CO3(s) + 2 HCl(aq) → 2 XCl(aq) + H2O(l) + CO2(g) How many moles of X2CO3 were consumed?
A student carried out the reaction below starting with 1.993 g of unknown (X2CO3), and found that the mass loss due to CO2 was 0.593 g. X2CO3(s) + 2 HCl(aq) → 2 XCl(aq) + H2O(l) + CO2(g) How many moles of X2CO3 were consumed?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 4PS: The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3(s) + 3 CO(g) 2...
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A student carried out the reaction below starting with 1.993 g of unknown (X2CO3), and found that the mass loss due to CO2 was 0.593 g.
X2CO3(s) + 2 HCl(aq) → 2 XCl(aq) + H2O(l) + CO2(g)
How many moles of X2CO3 were consumed?
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