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A sample of Cl2 with a pressure of 1.96 atm and a volume of 228 mL is allowed to react with excess Br2 at 114 °C. Br2 (g) + Cl2 (g) 2 BrCl (g) Calculate the pressure of the BrCl produced in the reaction if it is transferred to a 2.31-L flask and cooled to 36 °C. ___ atm

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Lelia LubowitzLv2
2 Oct 2019
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Related questions

At 400 K, the equilibrium constant for the reaction

Br2 (g) + Cl2 (g) <-----> 2BrCl (g)

is Keq = 7.0. A closed vessel at 400 K is charged with 1.00 atm ofBr2 (g), 1.00 atm of Cl2 (g), and 2.00 atm of BrCl (g). Use Q todetermine which of the statements below is true.

a. The equilibrium partial pressures of Br2, Cl2, and BrCl will bethe same as the initial values.
b. The equilibrium partial pressure of Br2 will be greater than1.00 atm.
c. At equilibrium, the total pressure in the vessel will be lessthan the initial total pressure.
d. The equilibrium partial pressure of BrCl (g) will be greaterthan 2.00 atm.
e. The reaction will go to completion since there are equal amountsof Br2 and Cl2.


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A researcher fills a 1.00 L reaction vessel with 2.80 x 10 ^-5 mol of BrCl gas and heats it to 500 K. At equilibrium, 8.12% of the BrCl gas remains. Calculate the equilibrium constant, Kc, assuming the following reaction: BrCl (g) <--> Br2 (g) + Cl2 (g).

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