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H2(g) + CO2(g) H₂O(g) + CO(g) Solution First we will set up an equilibrium table. It is important to understand how to set up this table, because we will use this throughout the course. Steps to set up an equilibrium table. 1) Set up table format, it is always the same. Initial (1) Change (C) Equilibrium (E) Initial (I) Change (C) Equilibrium (E) H2(g) + CO2(g) 2) Fill in the initial concentrations from the given information in the problem. H2(g) + Ş 1M Initial (I) Change (C) Equilibrium (E) H2(g) + 1M CO2(g) IM -X 3) To determine the change, you subtract "x" multiplied by the stoichiometric coefficient from the non-zero concentrations, and add "x" multiplied by the stoichiometric coefficients to the zero concentrations. This is the procedure to use only when we have zero concentrations of products or reactants. ↓↑ CO2(g) IM H₂O(g) + CO(g) -X H₂O(g) + CO(g) 0 0 H₂O(g) + CO(g) 0 0 +x + X

H2(g) + CO2(g) H₂O(g) + CO(g) Solution First we will set up an equilibrium table. It is important to understand how to set up this table, because we will use this throughout the course. Steps to set up an equilibrium table. 1) Set up table format, it is always the same. Initial (1) Change (C) Equilibrium (E) Initial (I) Change (C) Equilibrium (E) H2(g) + CO2(g) 2) Fill in the initial concentrations from the given information in the problem. H2(g) + Ş 1M Initial (I) Change (C) Equilibrium (E) H2(g) + 1M CO2(g) IM -X 3) To determine the change, you subtract "x" multiplied by the stoichiometric coefficient from the non-zero concentrations, and add "x" multiplied by the stoichiometric coefficients to the zero concentrations. This is the procedure to use only when we have zero concentrations of products or reactants. ↓↑ CO2(g) IM H₂O(g) + CO(g) -X H₂O(g) + CO(g) 0 0 H₂O(g) + CO(g) 0 0 +x + X

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 40GQ: Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample...
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ICE part 1,2,3 please. Tysm
Carbon monoxide in the following equilibrium reaction. If the initial concentration of both reactant carbon dioxide to produce water and gases is 1M, what is the final concentration of each gas in the reaction container? H2(g) + CO2(g) H₂O(g) + CO(g) Solution First we will set up an equilibrium table. It is important to understand how to set up this table, because we will use this throughout the course. Steps to set up an equilibrium table. 1) Set up table format, it is always the same. H2(g) + Initial (I) Change (C) Equilibrium (E) Initial (I) Change (C) Equilibrium (E) 2) Fill in the initial concentrations from the given information in the problem. H2(g) + CO2(g) 1M 1M Initial (I) Change (C) Equilibrium (E) CO2(g) H2(g) + 1M -X 3) To determine the change, you subtract "x" multiplied by the stoichiometric coefficient from the non-zero concentrations, and add "x" multiplied by the stoichiometric coefficients to the zero concentrations. This is the procedure to use only when we have zero concentrations of products or reactants. + CO2(g) IM -X H₂O(g) + CO(g) + H₂O(g) + CO(g) 0 0 H₂O(g) + CO(g) 0 0 +x + X
Transcribed Image Text:Carbon monoxide in the following equilibrium reaction. If the initial concentration of both reactant carbon dioxide to produce water and gases is 1M, what is the final concentration of each gas in the reaction container? H2(g) + CO2(g) H₂O(g) + CO(g) Solution First we will set up an equilibrium table. It is important to understand how to set up this table, because we will use this throughout the course. Steps to set up an equilibrium table. 1) Set up table format, it is always the same. H2(g) + Initial (I) Change (C) Equilibrium (E) Initial (I) Change (C) Equilibrium (E) 2) Fill in the initial concentrations from the given information in the problem. H2(g) + CO2(g) 1M 1M Initial (I) Change (C) Equilibrium (E) CO2(g) H2(g) + 1M -X 3) To determine the change, you subtract "x" multiplied by the stoichiometric coefficient from the non-zero concentrations, and add "x" multiplied by the stoichiometric coefficients to the zero concentrations. This is the procedure to use only when we have zero concentrations of products or reactants. + CO2(g) IM -X H₂O(g) + CO(g) + H₂O(g) + CO(g) 0 0 H₂O(g) + CO(g) 0 0 +x + X
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