Question

Carbon dioxide can be reacted with hydrogen to produce carbon monoxide and water. Write the balanced equation for this entirely gas-phase reaction:

Balance Equation:____________

At a temperature of 405 ?, this reaction has a pressure equilibrium constant of ?? = 1.44. Consider a system held at this temperature where the initial pressures of hydrogen, carbon dioxide, water vapor, and carbon monoxide are each equal to 0.40 atm. Will this reaction proceed in the forward or reverse direction upon equilibration? ___________________

In the space below and on the following page, calculate the equilibrium pressures of all molecular species, given the above initial conditions:

??O2,?q = ___________ ??2,?q =___________ ??2?,?q =___________ ??O,?q =___________

Explain below how the equilibrium constant here would be different for this reaction if it were performed in the aqueous phase. (Consider water in the aqueous phase, and recall the rules for equilibrium constants involving pure solids and liquids…)

Answer 1