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The following reaction reaches equilibrium at 350 degree C and 2 bar, with an equilibrium constant...

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.

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Expert Solution

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

queen_honey_blossom answered 1 year ago
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