1. The problem statement, all variables and given/known data A 10.0 g sample of solid platinum is placed in a large, sealed vessel at a sufficiently low pressure that the platinum is able to sublimate directly to a gas. Some thermodynamic properties of platinum at low pressure are given in the following table. Molar mass, M - 195 mol-1 Latent heat of sublimation, LS 363 kJ mol-1 Triple point pressure, pTP 3.50 Pa Triple point temperature, TTP 1550'C The platinum is heated at a rate of 10.0 W. If the initial temperature of the platinum is 25.0 ◦C, and it sublimates at the triple point temperature, how long will it take for the platinum to fully sublimate? 2. Relevant equations Q = nLS Q = mCT 3. The attempt at a solution My thoughts so far: Time = Energy required/power Energy required to sublimate at 1550"C = Q = nLS Energy required to heat from 25 - 1550 = Q = mcΔT. This is where i have a problem as there is no data given for the specific heat capacity of platinum. I was considering using the dulong-petit rule that all solids have Cv = 3R but the volume is not kept constant so I'm not sure how to work out the energy required to heat the platinum.