How much energy is removed when 45 grams of ethanol condenses to liquid? Ethanol heat of vaporization is ΔH(vap) 38.6 kJ/mol and heat of fusion is ΔH(fus) 4.60 kj/mol. Ethanol is 46. g/mol.

calculate the amount of heat in kilojoules needed to convert 95.65 grams of ice at 0.00 degree celcius to a gas.  The molar heat of fusion for ice is 6.02 kj/mol, the molar heat of vaporization is 40.6 kj/mol, and the specific heat of water is 4.184j/g degrees Celcius.

The following information is given for ethanol at 1 atm: Boiling point = 78.40°C Melting point =-114.5°C Specific heat gas = 0.3418 cal/g°C Specific heat liquid = 0.5880 cal/g°C Heat of vaporization = 200.0 cal/g Heat of fusion = 26.04 cal/g A 44.00 g sample of liquid ethanol is initially at -58.80°C. How many kcal of energy must be added to the sample to raise its temperature to 94.90°C? Energy added = kcal

Calculate the heat required to convert 22.2 g of propyl alcohol, C3H3O, from a solid at -141°C into the gaseous state at 115°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.

The heat of vaporization of water is 40.66 kJ/mol. How much heat is absorbed when 1.59 g of water boils at atmospheric pressure?.

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

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.

calculate the total amount of heat needed to convert 22.50 g of solid carbon tetrachloride, CCl4 at a temperature of -35 C to vapor form at 120 C, given the following values for CCl4 : melting point= -22.9 C; boiling point = 76.2C; change in H fusion = 2.69 kj/mol ; change in H vapor =29.8 kj/mol

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) ●