Objective: Using the equilibrium constant and reaction quotient expressions, and the ICEtable to calculate concentrations of various chemical species in the reaction.1. The water gas shift reaction (WGSR) has a K. = 2.7 at a given temperature:CO(g) + H₂O(g) — CO₂(g) + H₂(g)0.13 mol of CO, 0.56 mol of H₂O, 0.62 mol of CO2, and 0.43 mol of H₂ are placed in anevacuated 2.0 L flask.a. Prove or disprove that this is an equilibrium mixture, using the reaction quotient.b. Write an ICE (initial, change, equilibrium) table for the conditions given. Fill in the"change" line, consistent with your answer to part a.c. Solve the ICE table and write the equilibrium concentrations for all four chemicalspecies.d. The simplifying assumption that the change in concentration of the reactants isSMALL (and therefore negligible to the calculation) compared to the initial concentrationof the reactants. Is this assumption justified in this reaction and these conditions? Do alittle math to prove your point.

The reaction is: Number of moles of CO present = 0.13 molNumber of moles of H2O present = 0.56…

Answered: Objective: Using the equilibrium…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Objective: Using the equilibrium constant and reaction quotient expressions, and the ICE
table to calculate concentrations of various chemical species in the reaction.
1. The water gas shift reaction (WGSR) has a K. = 2.7 at a given temperature:
CO(g) + H₂O(g) — CO₂(g) + H₂(g)
0.13 mol of CO, 0.56 mol of H₂O, 0.62 mol of CO2, and 0.43 mol of H₂ are placed in an
evacuated 2.0 L flask.
a. Prove or disprove that this is an equilibrium mixture, using the reaction quotient.
b. Write an ICE (initial, change, equilibrium) table for the conditions given. Fill in the
"change" line, consistent with your answer to part a.
c. Solve the ICE table and write the equilibrium concentrations for all four chemical
species.
d. The simplifying assumption that the change in concentration of the reactants is
SMALL (and therefore negligible to the calculation) compared to the initial concentration
of the reactants. Is this assumption justified in this reaction and these conditions? Do a
little math to prove your point.

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d.The simplifying assumption that the change in concentration of the reactants is SMALL (and therefore negligible to the calculation) compared to the initial concentration of the reactants. Is this assumption justified in this reaction and these conditions? Do a little math to prove your point.

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