The following table gives the mole fraction of methylbenzene (A) in liquid and gaseous mixtures with...

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The following table gives the mole fraction of methylbenzene (A) in liquid and gaseous mixtures with butanone at equilibrium at XXXXXXXXXXK and the total pressure p. Take the vapour to be perfect and calculate the partial pressures of the two components. Plot them against their respective mole fractions in the liquid mixture and find the Henry’s law constants for the two components.

x_A	0	0.0898	0.2476	0.3577	0.5194	0.6036
y_A	0	0.0410	0.1154	0.1762	0.2772	0.3393
p/kPa	36.066	34.121	30.900	28.626	25.239	23.402
x_A	0.7188	0.8019	0.9105	1
y_A	0.4450	0.5435	0.7284	1
p/kPa	20.6984	18.592	15.496	12.295

David · Accepted Answer

We need to use :  pA=yAP and pB= yBP (Symbols have their usual meanings) 
Now we make the table for the x vs P plots.
pA /kPa         0     1.399      3.566    5.044     6.996      7.940    9.211     10.105      11.287      12.295
xA                  0     0.0898  0.2476   0.3577   0.5194  0.6036  0.7188  0.

The following table gives the mole fraction of methylbenzene (A) in liquid and gaseous mixtures with butanone at equilibrium at XXXXXXXXXXK and the total pressure p . Take the vapour to be perfect and...

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