Consider the endothermic decomposition of carbonic acid below H2CO3(aq) ⇌ CO2(g) + H2O(1) Where would the equilibrium shift if the volume of the system decreases at constant temperature?, and where would the equilibrium shift if N2 gas is introduced in the system?
Consider the endothermic decomposition of carbonic acid below H2CO3(aq) ⇌ CO2(g) + H2O(1) Where would the equilibrium shift if the volume of the system decreases at constant temperature?, and where would the equilibrium shift if N2 gas is introduced in the system?
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter16: Thermodynamics
Section: Chapter Questions
Problem 50E: Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial...
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Consider the endothermic decomposition of carbonic acid below
H2CO3(aq) ⇌ CO2(g) + H2O(1)
Where would the equilibrium shift if the volume of the system decreases at constant temperature?, and where would the equilibrium shift if N2 gas is introduced in the system?
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