Consider the decomposition of the compound C5H6O3 as follows C5H603 (g) --> C2H6

Question

Consider the decomposition of the compound C5H6O3 as follows
C5H603 (g) --> C2H6 (g) + 3CO (g)
When a 5.63g sample of pure C5H6O3 (g) was sealed into anotherwise empty 2.50-L flask and heated to 200C, the pressure inthe flask gradually rose to 1.63 atm and remained at that value. Calculate K for this reaction
C5H603 (g) --> C2H6 (g) + 3CO (g)
When a 5.63g sample of pure C5H6O3 (g) was sealed into anotherwise empty 2.50-L flask and heated to 200C, the pressure inthe flask gradually rose to 1.63 atm and remained at that value. Calculate K for this reaction

Explanation / Answer

Moles of C5H6O3 = mass / molar mass                               =5.63 g / 114.1 g/mol                               =0.05 moles . Pressure of C5H6O3 = n R T / V                                  = 0.05 moles * 0.0821 L-atm/ (mol.K) * (200+273) K / 2.50 L                                  = 0.78 atm This is the intitial pressure of C5H6O3 in the flask.                         C5H603(g) --> C2H6 (g) + 3CO (g) Initial(atm)          0.78                  0               0 Change(atm)         -x                     +x            +3x Equilibrium (atm) (0.78-x)             x               3x . Total pressure in the flask at equilibrium = 1.63 atm So 0.78-x + x + 3x = 1.63 atm x = 0.28 atm. . K = [p CO] 3 [p C2H6] / [p C5H6OH]     = (3x)3 * (x) / (0.78-x) Substituting the value of x and solving, we get K =0.405

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