When H2(g) is mixed with CO2(g) at 1750 K, equilibrium is achieved according to the following equation: CO2(g) + H2(g) ⇌ H2O(g) + CO(g). In one experiment, the following concentrations were measured: [H2] = 0.51 mol/L [CO2] = 0.53 mol/L [H2O] = 0.54 mol/L [CO] = 0.54 mol/L Calculate the value of the reaction quotient, Q. Note: Show all calculations, follow the rules of significant figures,
When H2(g) is mixed with CO2(g) at 1750 K, equilibrium is achieved according to the following equation: CO2(g) + H2(g) ⇌ H2O(g) + CO(g). In one experiment, the following concentrations were measured: [H2] = 0.51 mol/L [CO2] = 0.53 mol/L [H2O] = 0.54 mol/L [CO] = 0.54 mol/L Calculate the value of the reaction quotient, Q. Note: Show all calculations, follow the rules of significant figures,
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
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 15PS: The equilibrium constant for the dissociation of iodine molecules to iodine atoms I2(g) 2 I(g) is...
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18. When H2(g) is mixed with CO2(g) at 1750 K, equilibrium is achieved according to the following equation: CO2(g) + H2(g) ⇌ H2O(g) + CO(g). In one experiment, the following concentrations were measured:
[H2] = 0.51 mol/L [CO2] = 0.53 mol/L [H2O] = 0.54 mol/L [CO] = 0.54 mol/L Calculate the value of the reaction quotient, Q. Note: Show all calculations, follow the rules of significant figures, and box your final answer
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Show your understanding of the relationship between Keq and Q. If the reaction in #18, above, is at equilibrium when Keq = 4.0, explain whether or not the reaction is at equilibrium.
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