an 8.55mol saple of methanol, CH3OH, is placed in a 15.0L evacuated rigid tank and heated to 327 degrees Celsius. at temperature, all of the methanol is vaporized and some of the methanol decomposes to form carbon monoxide gas and hydrogen gas as represented in the equation CH3OH(g)-CO(g)+2H2(g)... (a) calculate the equilibrium constant for this reaction at 327degrees Celsius. identify if the equilibrium constant is Kc or Kp. (b) additional H2 is inserted to the equilibrium reaction at 327degrees Celsius. identify if the following will increase, decrease, or remain unchanged. justify each response. (i) the moles of CH3OH. (ii) the equilibrium constant.

Question

an 8.55mol saple of methanol, CH3OH, is placed in a 15.0L evacuated rigid tank and heated to 327 degrees Celsius. at temperature, all of the methanol is vaporized and some of the methanol decomposes to form carbon monoxide gas and hydrogen gas as represented in the equation CH3OH(g)->CO(g)+2H2(g)... (a) calculate the equilibrium constant for this reaction at 327degrees Celsius. identify if the equilibrium constant is Kc or Kp. (b) additional H2 is inserted to the equilibrium reaction at 327degrees Celsius. identify if the following will increase, decrease, or remain unchanged. justify each response. (i) the moles of CH3OH. (ii) the equilibrium constant.

jfraser · Answer

you can set up the equilibrium expression with the information given, but to calculate its $value$ you need to know $how much$ of the methanol has decomposed, or at least how much $CO$ or $H_2$ gas has formed. The rest is a simple ICE box approach