1. The problem statement, all variables and given/known data The bulb of a constant volume gas thermometer is immersed in an ice/water/water vapour mixture at equilibrium and the recorded pressure is 0.400 atm. It is then immersed in a boiling liquid and the pressure is 0.844 atm. Sufficient gas is then removed from the bulb such that, when the experiment is repeated, the gas pressures are 0.200 atm and 0.401 atm respectively. Calculate the boiling temperature of the liquid. 2. Relevant equations van der Waals equations of state are probably relevant here: [p + a(n/V)2][V - nb] = nRT ∴ [p + (a/Vm2)][Vm - b] = RT 3. The attempt at a solution I tried to arrange things better. If at first it was immersed in an "ice/water/water vapour mixture" then T = the triple point of water. So as I see it: V = constant T1 = 273.16 K, p1= 0.400 atm T2 = boiling point, p2 = 0.844 atm Some gas removed T1 = 273.16 K, p1= 0.200 atm T2 = boiling point, p2 = 0.401 atm Observations: From T1 to T2, the pressure of the gas doubles After the gas is removed, the pressure is halved, despite there being the same conditions is before I feel like the solution is in my head somewhere, but I've been rattling with it for eons without success. Any and all help very much appreciated.