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CaCO3(s): =CaO(s)+CO2(g), K = 0.058 at 727°C. A sample of 10.00 g of CaCO3 is placed in a 10.0L container at 727 °C. After equilibrium is reached, (a) what is the number of moles of CO₂ in the container, and (b) what mass of CaCO3 remains?

CaCO3(s): =CaO(s)+CO2(g), K = 0.058 at 727°C. A sample of 10.00 g of CaCO3 is placed in a 10.0L container at 727 °C. After equilibrium is reached, (a) what is the number of moles of CO₂ in the container, and (b) what mass of CaCO3 remains?

Chemistry & Chemical Reactivity
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
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section18.1: Spontaneity And Energy Transfer As Heat
Problem 2RC: A process that is reactant-favored at equilibrium can never be spontaneous. This statement is (a)...
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This is a part of the practice set for my exam. I keep having my questions returned saying they are graded. This is not graded I have the answers for these questions and need help with a step by step solution because I do not understand my professors explanation. Please help. THESE ARE NOT GRADED!
GC2.3.5 For the reaction CaCO3(s): = CaO(s)+CO,(g), K = 0.058 at 727°C. A sample of 10.00 g of CaCO3 is placed in a 10.0L container at 727 °C. After equilibrium is reached, (a) what is the number of moles of CO₂ in the container, and (b) what mass of CaCO3 remains?
Transcribed Image Text:GC2.3.5 For the reaction CaCO3(s): = CaO(s)+CO,(g), K = 0.058 at 727°C. A sample of 10.00 g of CaCO3 is placed in a 10.0L container at 727 °C. After equilibrium is reached, (a) what is the number of moles of CO₂ in the container, and (b) what mass of CaCO3 remains?
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