The reaction CO(g) + H20(g) CO2(g) + H2(g) has an equilibrium constant K, of 0.58 at 1000 °C. If a 60.0-L mixture of C0 and H,O has a concentration of each of 7.00×10-2 mol/L, wha amount (in moles) of each species will be present when the mixture reaches equilibrium? mol CO mol H20 mol CO2 mol H2 Submit Hide Tutor Steps
The reaction CO(g) + H20(g) CO2(g) + H2(g) has an equilibrium constant K, of 0.58 at 1000 °C. If a 60.0-L mixture of C0 and H,O has a concentration of each of 7.00×10-2 mol/L, wha amount (in moles) of each species will be present when the mixture reaches equilibrium? mol CO mol H20 mol CO2 mol H2 Submit Hide Tutor Steps
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![[Review Topics]
(References]
INTERACTIVE EXAMPLE Solving an Equilibrium Problem (Involving a Linear Equation in x)
The reaction
CO(g) + H2O(g)² C02(g) + H2(g)
has an equilibrium constant K¸ of 0.58 at 1000 °C. If a 60.0-L mixture of CO and H,O has a concentration of each of 7.00×10-² mol/L, what
amount (in moles) of each species will be present when the mixture reaches equilibrium?
mol CO
mol H20
mol CO2
mol H2
Submit
Hide Tutor Steps
TUTOR
The full ICE table is given here. The initial concentrations of CO and H,0 decrease by x mol/L and that of CO, and H, increase from zero
to x mol/L.
CO(g)
+ H20(g)
2 CO2(g) + H2(g)
Initial (M)
7.00x10-2
7.00×10-2
Change (M)
-X
+x
+x
Equilibrium (M) 7.00×102 - x 7.00×10-2 - x
Substitute the values for the equilibrium concentrations into the equilibrium constant expression and (using the known equilibrium constant
value) solve for the value ofx.
PROBLEM MAP
Previous
Ne](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe4d4a826-3cd8-448d-b0f0-2ac66e032b84%2F7b73eac6-fc34-4dee-ac87-b2051aa8b441%2Faku1d76_processed.jpeg&w=3840&q=75)
Transcribed Image Text:[Review Topics]
(References]
INTERACTIVE EXAMPLE Solving an Equilibrium Problem (Involving a Linear Equation in x)
The reaction
CO(g) + H2O(g)² C02(g) + H2(g)
has an equilibrium constant K¸ of 0.58 at 1000 °C. If a 60.0-L mixture of CO and H,O has a concentration of each of 7.00×10-² mol/L, what
amount (in moles) of each species will be present when the mixture reaches equilibrium?
mol CO
mol H20
mol CO2
mol H2
Submit
Hide Tutor Steps
TUTOR
The full ICE table is given here. The initial concentrations of CO and H,0 decrease by x mol/L and that of CO, and H, increase from zero
to x mol/L.
CO(g)
+ H20(g)
2 CO2(g) + H2(g)
Initial (M)
7.00x10-2
7.00×10-2
Change (M)
-X
+x
+x
Equilibrium (M) 7.00×102 - x 7.00×10-2 - x
Substitute the values for the equilibrium concentrations into the equilibrium constant expression and (using the known equilibrium constant
value) solve for the value ofx.
PROBLEM MAP
Previous
Ne
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