Use the van der waals equation to calculate the
pressureexerted by 1.000 mol of cl2 in 22.41 l at 273 k.
the van der waals constants for cl2 are: a =
6.49l2 atm/mol2 and b = .0562 l/mol.

P = 0.9885 atm

Explanation:

Van der Waals eq:

∴ Vm = 22.41 L / 1.000 mol = 22.41 L/mol

∴ R = 0.082 atm.L/Kmol

∴ T = 273 K

∴ a Cl2 = 6.49 L²atm/mol²

∴ b Cl2 = 0.0562 L/mol

⇒ P = ((0.082 atmL/Kmol)(273 K)/(22.41 L/mol - 0.0562 L/mol)) - ((6.49 L²atm/mol²)/(22.41 L/mol)²)

⇒ P = (1.0014 atm) - (0.013 atm)

⇒ P = 0.9885 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.