Final answer:
To calculate the pressure of Br2 at equilibrium, use the initial moles of Br2 and F2 using the ideal gas law. Then, use the stoichiometric coefficients in the balanced chemical equation to determine the change in moles at equilibrium. Finally, use the equilibrium constant expression to calculate the pressure of Br2 at equilibrium.
Step-by-step explanation:
To calculate the pressure of Br2 at equilibrium, we need to use the ideal gas law and the equilibrium constant (Kp) expression. First, let's calculate the initial moles of Br2 and F2 using the given pressures and the ideal gas law. We know that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
In this case, we are given the pressure and volume, so we can rearrange the equation to solve for n (the number of moles): n = (PV)/(RT).
Once we have the initial moles of Br2 and F2, we can use the stoichiometric coefficients in the balanced chemical equation to determine the change in moles at equilibrium. The equilibrium constant expression, Kp, is given as Kp = (P(BrF3)2)/(P(Br2)2 * P(F2)3)
We can use this expression to write an expression for P(Br2) in terms of Kp and the known pressures of BrF3 and F2. Finally, we substitute the values into the equation and solve for P(Br2).