In a 2.00 L sealed container at 373 K, pure nitrosyl bromide is introduced to a total pressure of 2.00 atm. The system reaches equilibrium according to
2NOBr(g)⇌2NO(g)+Br2(g).
At equilibrium the total pressure is 2.30 atm, and the partial pressure of Br2(g) is measured to be 0.30 atm.
Complete the following tasks, showing all reasoning.
(a) Determine the equilibrium partial pressures of NOBr(g) and NO(g).
(b) Calculate Kp for this reaction at 373 K.
(c) If the volume of the container is instantaneously doubled at 373 K, predict qualitatively how the partial pressures of all species will change as the system moves to a new equilibrium, and state whether the value of Kp will be altered. Justify your reasoning.