I need help with the following questions. If you don't have time to solve both then please do the 2nd one. The answers I got are 1a .5 1b 1 1c not sure how to do it 2a 3.86 2b 2.42^13 Are they correct? 1) For the following reaction 2SO2 + O2 <_-_-_-_-_-> 2SO3 What is the value of the Mass Action Expression when 2.5 moles of SO2 and 1.0 moles of O2 are placed in a 500mL container? What is the value after .50 moles of the O2 have been used up? What is the value at equilibrium if there is still 1.5 moles of O2 left? 4NH3 + 5O2 <_-_-_-_-_-> 4NO + 6H2O What is the value of the mass action expression in (d) above if, in a 2.5 liter container there is 7.5 moles of NH3, 5.0 moles of O2, 25.0 moles of NO and 2.5 moles of H2O? What is the value of the mass action expression if, at equilibrium, the concentration of the NO has increased to 11M?