Question

At 400 k, the equilibrium constant for the reaction br2 (g) + cl2 (g) 2brcl (g) is kp = 7.0. a closed vessel at 400 k is charged with 1.00 atm of br2 (g), 1.00 atm of cl2 (g), and 2.00 atm of brcl (g). use q to determine which of the statements below is true.
a.the equilibrium partial pressure of br2 will be greater than 1.00 atm.



b.the reaction will go to completion since there are equal amounts of br2 and cl2.



c.the equilibrium partial pressure of brcl (g) will be greater than 2.00 atm.



d.the equilibrium partial pressures of br2, cl2, and brcl will be the same as the initial values.



e.at equilibrium, the total pressure in the vessel will be less than the initial total pressure.

Answer 1

Answer:

(c) the equilibrium partial pressure of $BrCl(g)$ will be greater than $2.00$ atm.

Explanation:

Equilibrium constant of the given reaction will be as follows,

$Q_{p} =\frac{[products]}{[reactants]}$

Therefore, according to the equation

$Q_{p} = \frac{[2.00]^2}{{[1.00]}[1.00]}$

$Q_{p}= 4$

Since $K_{p}=7.0$

$Q_{p} < K_{p}$.

Since the reaction is moving n forward direction so the pressure will be increasing at equilibrium as compared to the initial pressure.

Also, the reaction is in equilibrium so it cannot be considered to be at completion.

So, option (c) the equilibrium pressure is of $BrCl(g)$ will be greater than $2.00$ atm is correct.