Suppose that a 1.0 liter vessel contains n2o gas at 1.0 atm pressure. suppose that a second vessel, 6.0 l in volume contains oxygen at 6.0 atm pressure. now suppose that the two vessels are connected by a pipe of negligible volume and the two gases mix and react to produce as much nitrogen dioxide as possible. assume that the temperature remains constant. what is the pressure in the apparatus at the end of the reaction?

P = 5.868 atm

Explanation:

assume T = 25°C = 298.15 K

∴ PN2O = 1 atm

∴ XN2O = nN2O/nt

∴ n = PV/RTideal gas

⇒ nN2O = ((1atm)(1L))/((0.082atm.L/K.mol)(298.15K)) = 0.041 mol N2O

∴ PO2 = 6 atm

∴ XO2 = nO2/nt

∴ nO2 = ((6atm)(6L))/((0.082atm.L/K.mol)(298.15K)) = 1.472 mol O2

⇒ nt = nN2O + nO2 = 0.041 + 1.472 = 1.513 mol

⇒ XN2O = 0.041/1.513 = 0.03

⇒ XO2 = 1.472/1.513 = 0.973

⇒ Pt = ((1atm)(0.03)) + ((6atm)(0.973))

⇒ Pt = 5.868 atm

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.