The reaction below takes place in a closed, rigid vessel. The initial pressure of N2(g) is 1.0 atm, and that of O2(g) is 1.5 atm. No N2O4(g) is initially present. The experiment is carried out at a constant temperature. What is the total pressure in the container when the partial pressure of N2O4 reaches 0.75 atm? N2+O2->N2O4

Please help and explain how you got the answer. I need help on got to get to the answer itself.

the correct answer is a

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.