What is the AS for the phase change of 2.00 moles of water from solid to liquid (A H = 6.01kJ

10. In which state (x) does a gram of water loses less heat to cool down to 20 °C? (1) at +40 °C or (1) at +50 °C (g with I) at +100 °C or (g) at +100 °C

53. What mass of water initially at -12.5 °C can be converted to liquid water at 27.9 °C by 38.36 kJ of energy? AHfus = 334 J/g AHvap =2261 J/g Csolid=2.11 J/g.°C Cliquid 4.18 J/g °C Cgas = 2.01 J/g °C A. 80.4 g B. 91.5 g C. 76.3 g D. 268 g =

• At its boiling point (-61 C), what mass of H2S is vaporized with 100 kJ? The AHvap of H2S, is 18.8 kJ/mol?

A certain liquid has a vapor pressure of 92.0 Torr at 23.0 °C and 259.0 Torr at 45.0 °C. Calculate the value of AHap for this liquid. AH vap = Calculate tl x10 boiling point: TOOLS s liquid. kJ/mol °C

How much energy is required to vaporize 41.4 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol?

Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.

From 25.0°C to 94.5°C, 75.1 grams of ethanol are heated. What was the energy requirement in joules?H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, and cp (solid) ethanol 2.42 J/g°C are the specific temperatures for the three phases of ethanol. Ethanol has a molecular weight of 46. The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.