Use the information in Tables 2D.1 and 2E.1 to calculate the energy that must be transferred as heat to melt 100 g of ice at 0 °c, increase the sample temperature to 100 °c, and then vaporize it at that temperature. Sketch a graph of temperature against time on the assumption that the sample is
heated at a constant rate.
Extracted text: Table 2D.1 Temperature dependence of heat capacities* Substance a/(J K-1 mol-1) b/(J K-² mol-1) c/J K mol-1) C(s, graphite) 16.86 4.77 x 10-3 -8.54 x 105 CO,(g) 44.22 8.79 x 10-3 -8.62 x 105 H,O(1) N2(g) 75.29 28.58 3.77 x 10-3 -5.0 x 104 Cu(s) 22.64 6.28 x 10-3 NaCl(s) 45.94 16.32 x 10-3 The constants are for use in eqn 6a (Cm = a+ bT+ c/T). Experimental values at 25 °C are listed in the Resource section.
Extracted text: Table 2E.1 Standard enthalpies of transition at the transition temperature* Substance Freezing point, T;/K AfugH°/(kJ mol-1) Boiling point, T,/K Avap H°/(kJ mol") Ammonia, NH3 195.3 5.65 239.7 23.4 Argon, Ar 83.8 1.2 87.3 6.5 Benzene, CHs Ethanol, C2H,OH 278.7 9.87 353.3 30.8 158.7 4.60 351.5 43.5 Helium, He 3.5 0.02 4.22 0.08 Mercury, Hg Methane, CH4 234.3 2.292 629.7 59.30 90.7 0.94 111.7 8.2 Methanol, CH,OH 175.5 3.16 337.2 35.3 Propanone, CH;COCH3 177.8 5.72 329.4 29.1 Water, H2O 273.15 6.01 373.2 40.7 * For values at 298.15 K, use the information in the Resource section. The transition temperatures are for 1 atm, but (except for very precise work) the values at 1 bar are negligibly different.