III.(24) Consider the reaction 2 NOBr(g) --> 2 NO(g)-+ Br2(g) (i) (12pts)At equilibrium, and a temperature of 100.0°C, a 5.00 liter flask contains 3.22 g of NOBr(g), 3.08 g of NO(g) and 4.19 g of Br2(g). Calculate Ko at this temperature (ii) (12pts)Calculate the reaction quotient Q if a 5.00 L at 100.0°C contains 0.040 moles of NOBr, 0.25 moles NO(g) and 0.025 moles Br2(g). Will the reaction shift to the right or left to establish equilibrium? IV.. (10 pts) Find the missing equilibrium constant. All data is at 1330 K 4 GeWO.(g) = 4 GeO(g) +2W,06(g) Gew,07(g) = GeO(g) W,06(g) 2 Gewo,(g) = GeO(g) + Gew,07(g) K,' = ? 2.041 x 10-8 K" = 2.63 x V. (10pts) For the equilibrium I2(g) + Br2(g)2 IBr(g) K. = 280.0 at 150.0°C . Suppose that 0.500 mol of IBr(g) is placed in a 3.00 L flask and allowed to reach equilibrium at this temperature. What are the equilibrium concentrations of I2(g), Br2(g), and IBr(g)?