Given the following data at a certain temperature, 2n2(g) + o2(g) + 2n2o(g) k=1.2 x 10-35 n204(g) + 2no2(g) k=4.6 x 10-3 12 n2(g) + o2 + no2(g) k-4.1 x 109 calculate k for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas. 7. for the system pcls(g) + pc13(g) + cl2(g) k is 26 at 300°c. in a 5.0-l flask, a gaseous mixture consists of all three gases with partial pressure as follows: ppcis = 0.012 atm, pcl2 = 0.45 atm, ppci3 = 0.90 atm. a) is the mixture at equilibrium? explain. b) if it is not at equilibrium, which way will the system shift to establish equilibrium? 8. for the reaction: n2(g) + 2h2o(g) + 2no(g) + 2h2(g) k is 1.54 x 10-3. when equilibrium is established, the partial pressure of nitrogen is 0.168 atm, and that of no is 0.225 atm. the total pressure of the system at equilibrium is 1.87 atm. what are the equilibrium partial pressures of hydrogen and steam?