Help with Equilibrium: CH4 + H2O -> CO + 3H2

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SUMMARY

The discussion focuses on the equilibrium state of the reaction CH4 + H2O <-----> CO + 3H2, where a chemical engineer analyzes the conversion of methane in a 0.32L flask at 1200 K. At equilibrium, the flask contains 0.26 mol of CO, 0.091 mol of H2, and 0.041 mol of CH4. The equilibrium constant, Kc, is given as 0.26. The primary question is to determine the concentration of H2O at equilibrium based on these values.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Knowledge of equilibrium constant (Kc) calculations
  • Familiarity with stoichiometry in chemical reactions
  • Basic skills in molarity and concentration calculations
NEXT STEPS
  • Calculate the concentration of H2O at equilibrium using the Kc expression
  • Review the principles of chemical equilibrium and Le Chatelier's principle
  • Explore the implications of temperature on equilibrium constants
  • Study the effects of varying concentrations on reaction shifts
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Chemical engineers, chemistry students, and researchers involved in reaction kinetics and equilibrium studies will benefit from this discussion.

apiwowar
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In a study concerning the conversion of methane to other fuels, a chemical engineer mixes gaseous CH4 and H2O in a 0.32L flask at 1200 K. At equilibrium the flask contains 0.26 mol of CO, 0.091 mol of H2, and 0.041 mole of CH4. What is the [H2O] at equilibrium? Kc=0.26 for the eqtn
annnd the eqtn is CH4 + H2O <-----> CO + 3H2

have no idea how to do this, any tips or help?
 
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If you would try to follow template, you would have the answer ready.

What is the equation for Kc for this reaction?

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methods
 

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