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The equilibrium constant in terms of pressures for the reaction C6H5CH2OH(g) <--> C6H5CHO(g) + H2(g) is...

The equilibrium constant in terms of pressures for the reaction C6H5CH2OH(g) <--> C6H5CHO(g) + H2(g) is Kp = 0.558 at 523 K.

(a) A pure sample of gaseous benzyl alcohol, C6H5CH2OH(g), is introduced into a rigid flask at a temperature of 523 K so that its original pressure is 0.126 atm. Calculate the fraction of this starting material that is converted to products at equilibrium.

(b) A second sample of benzyl alcohol is introduced into a rigid flask at a temperature of 523 K, this time at an original pressure of 4.96 atm. Again, calculate the fraction of the starting material that is converted to products at equilibrium.

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While solving the problem I have expressed partial pressure of a particular compound with "p" with the structure of the compound in the subscript.

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