Consider the following exothermic reaction: If you were a chemist trying to maxi

Question

Consider the following exothermic reaction:

If you were a chemist trying to maximize the amount of C2H4Cl2 produced, which of the following might you try? Assume that the reaction mixture reaches equilibrium.

A)  condense C2H4Cl2 as a pure liquid from the reaction mixture

B)  decrease the total pressure

C)  increase the total pressure

D)  raise the temperature

E)  both A and C

The reaction below has an equilibrium constant of

What is the value of Kp for the reaction below? AND Will the reaction products or reactants be favored at Equilibrium?

A)  Kp = -2.26

Consider the following exothermic reaction: If you were a chemist trying to maximize the amount of C2H4Cl2 produced, which of the following might you try? Assume that the reaction mixture reaches equilibrium. condense C2H4Cl2 as a pure liquid from the reaction mixture decrease the total pressure increase the total pressure raise the temperature both A and C The reaction below has an equilibrium constant of What is the value of Kp for the reaction below? AND Will the reaction products or reactants be favored at Equilibrium? Kp = -2.26 times 104 ; Products are favored Kp = 4.4 times 10-4 ; Reactants are favored Kp = 6.7 times 10-3.; Products are favored Kp = 6.7 times 10-3.; Reactants are favored Kp = 1.5 times 102 ; Products are favored

Explanation / Answer

E) both A and C

new Kp = 1/square root of (K'p)
where K'p = 2.26*10^4
new Kp = 0.665*10^-2 = 6.67*10^-3 : reactents are favored(when Qp >Kp)

                    

6.67*10^-3 : productss are favored(when Qp < Kp)

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