At 400 K, the equilibrium constant (Kp) for the reaction Br2(g) + Cl2(g) 2 BrCl(
ID: 945758 • Letter: A
Question
At 400 K, the equilibrium constant (Kp) for the reaction Br2(g) + Cl2(g) 2 BrCl(g) is 5.6 x 10^3 . A closed vessel at 400 K is charged with 1.00 atm of Br 2 (g) , 1.00 atm of Cl 2 (g) , and 2.00 atm of BrCl(g) . Which of the following is true?
A. The equilibrium partial pressures of Br 2 ,Cl 2 , and BrCl will be the same as the initial values.
B. The equilibrium partial pressure of Br 2 will be greater than 1.00 atm.
C. At equilibrium, the total pressure in the vessel will be less than the initial total pressure.
D. The equilibrium partial pressure of BrCl(g) will be greater than 2.00 atm. E. The reaction will go to completion since there are equal amounts of Br 2 and Cl 2 .
Explanation / Answer
The equilibrium partial pressure of BrCl(g) will be greater than 2.00 atm.
Because
Br2(g) + Cl2(g) 2 BrCl(g) is Kp = 5.6 x 10^3
where as for backward reaction 2 BrCl(g) Br2(g) + Cl2(g) Kp = 1/(5.6 x 10^3)
it indicates that farward is more faster than reverse reaction
therefore more amount of Br2(g) and Cl2(g) will be converted into BrCl(g)
it results the equilibrium partial pressure of BrCl(g) will be greater than 2.00 atm.
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