Consider the following reaction (assume an ideal gas mixture): 2NOBr(g) + 2NO(g) Br2(g)
A 1.0-liter vessel was initially filled with pure NOBr, at a pressure of 4.0 atm, at 300 K. After equilibrium was reached, the volume was increased to 2.0 liters, while the temperature was kept at 300 K. The result of this change was:
a. a shift in the equilibrium position to the right.
b. an increase in Kp.
c. a shift in the equilibrium position to the left.
d. a decrease in Kp.
e. None of these choices are correct.