A mixture containing C5H6, HCl, Cl2, and C5H8, all at an initial partial pressure of 4.74 atm, is allowed to achieve equilibrium according to the equation below. At equilibrium, the partial pressure of C5H8 is observed to have decreased by 0.82 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)

To solve this problem, we need to understand the concept of equilibrium and the equilibrium constant (Kp).

The equilibrium constant expression for the given reaction is:

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

Given that the initial partial pressure of all gases is 4.74 atm, and the partial pressure of C5H8 decreases by 0.82 atm at equilibrium, we can infer that the partial pressure of C5H6 also decreases by 0.82 atm (since the reaction consumes C5H6 to produce C5H8).

The change in the partial pressure of HCl is twice that of C5H6 or C5H8 (since the stoichiometric coefficient of HCl is 2), so the partial pressure of HCl decreases by 2*0.82 = 1.64 atm.

The change in the partial pressure of Cl2 is equal to the change in the partial pressure of C5H8 (since they are produced in a 1:1 ratio), so the partial pressure of Cl2 increases by 0.82 atm.

At equilibrium, the partial pressures of the gases are:

[C5H6] = 4.74 - 0.82 = 3.92 atm [HCl] = 4.74 - 1.64 = 3.10 atm [Cl2] = 4.74 + 0.82 = 5.56 atm [C5H8] = 4.74 - 0.82 = 3.92 atm

Substituting these values into the equilibrium constant expression gives:

Kp = (3.92 * 5.56) / (3.92 * 3.10^2) = 0.175

So, the equilibrium constant Kp for this reaction is approximately 1.75 x 10^-1 (to 3 significant figures in scientific notation).