Question

A mixture containing C5H6, HCl, Cl2, and C5H8, all at an initial partial pressure of 4.95 atm, is allowed to achieve equilibrium according to the equation below. At equilibrium, the partial pressure of C5H8 is observed to have decreased by 0.37 atm.

Determine Kp for this chemical equilibrium. Report your answer to 3 significant figures in scientific notation.

C5H6(g) + 2HCl(g) ⇌ Cl2(g) + C5H8(g)

Answer 1

Initially

C5H6 = 4.95

HCl = 4.95

Cl2 = 4.95

C5H8 = 4.95

in equilbirium (according to sotichiometry)

C5H6 = 4.95 - x

HCl = 4.95 -2x

Cl2 = 4.95 +x

C5H8= 4.95 + x

Since C5H8 in equilibrium = 0.37

then

4.95 + x = 0.37

x = 0.37-4.95 = -4.58

meaning that there is actually production of reactants

K must be < 1; since it f

calculate all concnetrations

C5H6 = 4.95 - x = 4.95+4.58 = 9.53

HCl = 4.95 -2x = 4.95+2*4.58 = 14.11

Cl2 = 4.95 +x = 4.95-4.58 = 0.37

C5H8= 4.95 + x = 0.37

Apply Kp

Kp = [Cl2][C5H8]/([C5H6][HCl]^2)

Kp = (0.37)(0.37)/(9.53*(14.11^2))

then

Kp = 0.00007215335

Kp = 7.21*10^-5