Given the equilibrium constants for the following two reactions in aqueous solution at 25 C, HNO2 (aq) + H+(aq) + NO2 (aq) Kc = 4.5 x 10-4 H2SO3(aq) + 2 H+ (aq) + SO3- (aq) Kc= 1.1 x 10-9 what is the value of Kc for the reaction? 2 HNO3(aq) + Soz-(aq) H2SO3(aq) + 2 NO2 (aq) 2. Given that, at 700 K, Kp = 54.0 for the reaction: H2(g) + 12(g) 2 HI(g) and Kp = 1.04 x 10-4 for the reaction: N2(g) + 3H2(g) 6 2 NH3(g) determine the value of Kp for the reaction 2 NH3(g) + 312(g) + 6 HI(g) + N2(9) at 700 K. 3. The gaseous compound BrCl decomposes at high temperature in a sealed container: 2 BrCl(g) Br2(g) + Cl2(g). Initially, the vessel is charged at 500 K with BrCl(g) at a partial pressure of 0.500 atm. At equilibrium, the BrCl(8) partial pressure is 0.040 atm. Calculate the value of Kp at 500 K