The water gas shift reaction involves the reaction of carbonmonoxide with water vapor to form carbon dioxide and hydrogengas:
CO(g) + H2O(g) → CO2(g) +H2(g)
28.01 g CO and 9.01 g water vapor are combined in a reactionvessel. At the end of the reaction, a total pressure of 945.3 torris found.
A.) Which gases are left at the end of the reaction?
B.) What are mole fractions of the gases left in the reactionvessel after the reaction? Clearly identify which mole fractionbelongs to which gas, and report all mole fractions to threesignificant figures.
C.) What is the actual volume of the reaction vessel if thereaction from Question 1 occurred at 115.0oC? Give youranswer with the correct unit. Hint: you should be able to find themoles of all gases from the data given.
D.) If the volume of the reaction vessel is somehow changed to55.3 L at constant temperature, what will the new total pressure ofthe gas mixture (after the reaction in Question 1) be? Give youranswer to the correct number of significant figures and unit.
