MORE HEAT PRACTICE The data below refers to an unknown substance, X. Boiling Point Heat of Fusion Heat of Vaporization SH Capacity SH (solid) (liquid) 425 kJ/g 695 kJ/g 2.3 J/gºC 5.9 3/gºC 1.1 3/gºC 1. Draw a heating curve for substance X, going from 15°C to 125°C on the axis below. Write in all formulas used to calculate heat. Melting point 32.0°C 112.0°C SH (vapor) b. Determine the amount of heat released when 15.0g of gaseous X at 112.0°C changes to liquid at 112.0°C. 9 AH

How much heat (in kJ) would need to be removed to cool 189.9 g of water from 25.60°C to -10.70°C? Csolid = Cliquid = 2.092 J/g-°C 4.184 J/g C AHrusion = Trusion = 0.0 °C 6.01 kJ/mol A events.ics D CertainGovernm.pdf D CertainGovernm.pdf D 2020 W-2 and E.pdf 888

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

How much heat would need to be removed to cool 50.3 g of water from 25.6°C to -10.7°C? Csolid = 2.092 J/g °C Tfusion = 0.00 °C Cliquid = 4.184 J/g °C AHfusion = 6.01 kJ/mol

O Macmillan Learning How much heat energy is required to convert 51.4 g of solid ethanol at -114.5 °C to gaseous ethanol at 135.7 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g °C, and that of gaseous ethanol is 1.43 J/g °C. 9 = kJ

Calculate the heat energy released when 19.8 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for mercury at 1 atm kJ heat capacity of Hg(1) 28.0 J/(mol·K) と TOOLS x10 melting point 234.32 K enthalpy of fusion 2.29 kJ/mol

How much heat is required to warm 25.0 g of H2O from a solid at -12ºC to a liquid at 60ºC? ∆Hfus = 6.02 kJ/mol Csolid = 2.09 J/gºC Cliq = 4.18 J/gºC Tfreezing = 0ºC

When 95.0 grams of ethanol condenses to liquid, how much energy is lost? H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. Ethanol has a molecular weight of 46.

How much energy (in kļ) is needed to heat 5.03 g of ice from -20.3°C to 30.0°C? The heat of fusion of water is 6.01 kJ/(mol), and the heat capacity is 2.093 J/(g °C) for ice and 4.184 J/(g °C) for liquid water. Your answer should have 3 sig figs. Answer:

How many joules are needed to vaporize 125 g of liquid water at 100°C? The latent heat of vaporization is 2258 J/g. 2.82 J282,000 J282 J2,820,000 J