Ethanol (C2H5OH) melts at -114 oC and boils at 78 oC. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol the specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat is required to convert 31.55 g of ethanol at -200 oC to the vapor phase at 78 oC? (Give your answer in unit of kilojoules)

What quantity of heat is required to convert 49 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)

Ethanol (C₂H₂OH) meits at-114 °C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Y Part A How much heat is required to convert 30.5 g of ethanol at 28 °C to the vapor phase at 78 "C? Express your answer in kilojoules to three significant figures. 195] ΑΣΦ Submit Part 8 Request Answer Submit ? How much heat is required to convert 30.5 g of ethanol at-160 C to the vapor phase at 78 "C7 Express your answer in kilojoules to two significant figures. VA24 Request Answer kJ kJ

The following information is given for cobalt at 1atm: boiling point = 3097°C AHvap = 6.60 kJ/g melting point = 1495°C AHfus = 263 J/g What is the energy change, Q, in kJ for the process of freezing a 39.8 g sample of liquid cobalt at its normal melting point of 1495°C. kJ

Ethanol (C2 H5 OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? 3949 207.3 6.67 8.97 -12.5

Carbon tetrachloride (CCl4) boils at 77∘C. The measured enthalpy of vaporization is 29.8 kJ/mol What is the heat of vaporization?

How much heat (q) in joules (J) was involved when 52.4 g of steam was condensed  (DHvapH2O = 2260 J/g) with a phase change at the boiling point of water?

What quantity of heat, in kJ, is required to convert 12.0 g of ethanol (C₂H₂OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g C; AHvap = 39.3 kJ/mol) ●

Consider the following data for ethanol, C2H5OH: Melting Point = -114°C Boiling Point = 78°C ΔHfusion = 5.0 kJ/mol ΔHvaporization = 42.6 kJ/mol Specific Heat of Liquid Ethanol = 2.5 J/g•°C Sketch a cooling curve that depicts ethanol vapor at 78°C being cooled until solid ethanol is formed at -114°C and then calculate the total amount of heat in kilojoules released when 55 grams of ethanol undergoes this process.

How much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJ