CHEM 104 Homework 5 3. 20 points-Ch. 17.6 Methanol (CH.OH) is a liquid fuel and
ID: 1024935 • Letter: C
Question
CHEM 104 Homework 5 3. 20 points-Ch. 17.6 Methanol (CH.OH) is a liquid fuel and solvent that can be produced by the reaction of syngas (Co and Ha). If the reaction is run below the boiling point of methanol, the equilibrium reaction is as follows: At 298 K, an equilibrium mixture in a 100-L test reactor was found to contain the following partial pressures: Poo-0.0223 atm, and P%-0.0446 atm. a) Calculate the value of the equilibrium constant K b) Additional reactants are then pumped into the reactor, doubling the CO and H: partial pressures. When equilibrium is reestablished, how many moles of additional methanol will have been produced? Suggest two ways that an engineer might improve the yield of methanol produced by this reaction. c)Explanation / Answer
a) kp=1/[(pco)x(pH2)2]..........(1)
kp=1/(0.0223x(0.0446)2)=22543.712
b) after doubling partial pressure of CO and H2,
the pressure of CO becomes 2x0.0223=0.0446atm,pressure of H2 becomes 2x0.0446=0.0892
at new equilibrium Pco=0.0446-x ,PH2=0.0892-2x and methanol obtained is x
kp will remain same as temperature is same.so kp=22543.712
using equation (1) and placing value of Pco and PH2,we obtain 22543.712=1/[(0.0446-x)(0.0892-2x)2]
by solving the above equation value of x can be calculated and value of x will give amount of methanol formed
c) as n.of moles at product side is less,so on increasing pressure ,equilibrium will shift in forward direction according to Le chatlier principle.On increasing temperature .equilibrium will shift in backward direction due to exothermic reaction.so,best yield of methanol can be obtained at low temperature and high pressure.