In: Chemistry
The following reaction reaches equilibrium at 350 degree C and 2 bar, with an equilibrium constant K = 3.7064 at these conditions: C H subscript 3 C H O space left parenthesis g right parenthesis space plus space H subscript 2 space left parenthesis g right parenthesis space rightwards arrow space C subscript 2 H subscript 5 O H space left parenthesis g right parenthesis If the system initially contains 1 mol of H2 and 1 mol of acetaldehyde, what is the extent of reaction? Assume ideal gases. Give your answer to 2 decimal places.
For the reaction given:
Keq = 3.7064
CH3CHO(g) +
H2(g)
C2H5OH(g)
Initial
1
1
0
Change
-x
-x
+x
Equilibrium
1 -
x
1 -
x
x
Keq = [C2H5OH] / [CH3CHO][H2]
3.7064 = x / (1-x)(1-x)
x = 0.598
At equilibrium:
CH3CHO = 1 - 0.598 = 0.402
H2 = 1 - 0.598 = 0.402
C2H5OH = 0.508
Extent of reaction,
= ni / vi
where, ni is the moles of the i-th reactant and νi is the stoichiometric number of the i-th reactant.
= (0.402 - 1) / (-1)
= 0.59