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Consider the gas phase reaction below: CO (g) + H2O (g) → CO2 (g) + H2 (g) The value of the equilibrium constant, Ke, is 1.845 at a given temperature. If 2.30 mol of CO and 2.30 mol of H2O are placed in a 5.00 L container at this temperature, what will be the concentration of carbon monoxide after equilibrium is reached? Hint: Use an ICE table and avoid the quadratic equation by recognizing there is a "perfect square" (see p. 677 in our textbook). a) b) 0.104 M 0.0873 M d) 0.195 M 0.265 M e) 0.377 M

Consider the gas phase reaction below: CO (g) + H2O (g) → CO2 (g) + H2 (g) The value of the equilibrium constant, Ke, is 1.845 at a given temperature. If 2.30 mol of CO and 2.30 mol of H2O are placed in a 5.00 L container at this temperature, what will be the concentration of carbon monoxide after equilibrium is reached? Hint: Use an ICE table and avoid the quadratic equation by recognizing there is a "perfect square" (see p. 677 in our textbook). a) b) 0.104 M 0.0873 M d) 0.195 M 0.265 M e) 0.377 M

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 51QAP: . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular...
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9. Consider the gas phase reaction below: CO (g) + H2O (g) → CO2 (g) + H2 (g) The value of the equilibrium constant, Ke, of CO and 2.30 mol of H20 are placed in a 5.00 L container at this temperature, what will be the concentration of carbon monoxide after equilibrium is reached? Hint: Use an ICE table and avoid the quadratic equation by recognizing there is a "perfect square" (see p. 677 in our textbook). 1.845 at a given temperature. If 2.30 mol 0.0873 M a) b) 0.195 M d) e) 0.265 M 0.377 M 0.104 M Consider the heterogeneous reaction below: Cl2(H2O)8 (s) → Cl2 (g) + 8H2O (g) When solid Cl2(H2O)8 is placed in a 20.0 L container at -10. °C, the equilibrium partial pressure of water vapor produced is 5.34 x 103 atm. 0. What's the equilibrium partial pressure of chlorine gas, Cl2? Hint: Use an ICE table and al states.
Transcribed Image Text:9. Consider the gas phase reaction below: CO (g) + H2O (g) → CO2 (g) + H2 (g) The value of the equilibrium constant, Ke, of CO and 2.30 mol of H20 are placed in a 5.00 L container at this temperature, what will be the concentration of carbon monoxide after equilibrium is reached? Hint: Use an ICE table and avoid the quadratic equation by recognizing there is a "perfect square" (see p. 677 in our textbook). 1.845 at a given temperature. If 2.30 mol 0.0873 M a) b) 0.195 M d) e) 0.265 M 0.377 M 0.104 M Consider the heterogeneous reaction below: Cl2(H2O)8 (s) → Cl2 (g) + 8H2O (g) When solid Cl2(H2O)8 is placed in a 20.0 L container at -10. °C, the equilibrium partial pressure of water vapor produced is 5.34 x 103 atm. 0. What's the equilibrium partial pressure of chlorine gas, Cl2? Hint: Use an ICE table and al states.
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