An evacuated 1.000 L flask was filled at room temperature with 0.01308 mol NO (nitrogen monoxide) and 0.00559 mol Br2 (bromine). The temperature was then raised to 50.5°C, and these substances reacted to give nitrosyl bromide, NOBr: 2NO(g) + Brz (g)=2NOBr (g) Given that when the equilibrium was achieved, the pressure of the gases in the flask was found to be 0.4027 atm. a) Calculate the total moles (in four significant figures) of gases in the flask at equilibrium. [6 marks) b) Calculate the number of moles (in three significant figures) for each substance that formed in the flask at equilibrium. [6 marks] c) Calculate the partial pressures (in three significant figures) of the different gases and K, (in three significant figures) in this equilibrium mixture. [8 marks]