Question

An evacuated 1.000 L flask was filled at room temperature with 4.920E-2 mol NO (nitrogen monoxide) and 7.74E-3 mol Br₂ (bromine). The temperature was then raised to 50.5°C, and these substances reacted to give nitrosyl bromide, NOBr:

2NO(g) + Br(g) <--> 2NOBr(g)

When equilibrium was achieved, the pressure of the gases in the flask was found to be 1.315 atm.

(a) What was the total moles of gases in the flask at equilibrium?	ntotal = mol
(b) How many moles of nitrosyl bromide were formed? What was the moles of each substance in the flask at equilibrium?	n(NO) = mol n(Br2) = mol n(NOBr) = mol
(c) What are the partial pressures of the different gases in this equilibrium mixture?	p(NO) = atm p(Br2) = atm p(NOBr) = atm
(d) What is Kp at this temperature?	Kp =