The reaction system represented above is at equilibrium. Which of the following will decrease the amount of CaO(s)in the system?

(A) Increasing the volume of the reaction vessel at constant temperature

(B) Lowering the temperature of the system

(C) Removing some CO2(g)at constant temperature

(D) Removing someCaCO3(s)at constant temperature

Steam reforming of methane ( ch4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. an industrial chemist studying this reaction fills a 1.5 l flask with 3.5 atm of methane gas and 1.3 atm of water vapor at 43.0°c. he then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 1 .0 atm. calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. round your answer to 2 significant digits.