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A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH₂OH(g) CO(g) + 2 H₂(g), Kc = 6.90 x10-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?

A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH₂OH(g) CO(g) + 2 H₂(g), Kc = 6.90 x10-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?

Chemistry
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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A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g) = CO(g) + 2 H₂(g), Kc = 6.90 ×10-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?
Transcribed Image Text:A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500 K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g) = CO(g) + 2 H₂(g), Kc = 6.90 ×10-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M, what mass of methanol was initially introduced into the vessel?
Expert Solution
Step 1

First we need to calculate the initial molarity of methanol using the Kc value and equilibrium concentration of H2 . 

Using concentration and volume, we can calculate moles of methanol. 

Then we can convert moles to mass using molar mass. 

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