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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Patrina SchowalterLv2

31 Dec 2019

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At 298 K, 1.30 mol BrCl(g) is introduced into a 12.0 âL vessel, and equilibrium is established in the reaction.
BrCl(g)â0.5Br2(g)+0.5Cl2(g):

1.Calculate the amount of BrCl(g) present when equilibrium is established. [Hint: Use ÎG0[Br2(g)]=3.11kJ/mol, ÎG0[BrCl(g)]=â0.98kJ/mol.]

2.Calculate the amount of Br2(g) present when equilibrium is established.

3.Calculate the amount of Cl2(g) present when equilibrium is established.

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.

The reaction of bromine gas with chlorine gas, shown here, has a Kc value of 7.20 at 200ºC. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.200 M, but with no initial concentration of BrCl, what would be the equilibrium concentration of BrCl(g)?

Br2(g) + Cl2(g)= 2BrCl(g) K = 7.20
Initial Concentrations 0.20 0.20 0