Answer:-
Firstly from the given mass and molar mass , moles are calculated then using enthalpy of vaporisation, energy is calculated.
The answer is given in the image,
How much energy is required to vaporize 158 g of butane that has already been brought...
How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point, if its ΔHvap is 24.3 kJ/mol
How much energy is required to vaporize 175 g of butane at its boiling point? The heat of vaporization for butane is 23.1 kJ/mol. Express your answer to three significant figures and include the appropriate units.
53) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its AHvap is 31.6 kJ/mol? A) 31.2 kJ B) 6.49 kJ C) 18.1 kJ D) 55.1 kJ E) 15.4 kJ
How much energy is required tp vaporize 48.7 g pf dichloromethane at its boiling point, if tis Hvap is 31.6 kJ/mol?
How much energy is needed to vaporize 230.0 g of liquid benzene (C6H6) at its boiling point? The molar heat of vaporization of benzene is 33.83 kJ/mol.
How much heat must be added to vaporize 245 g of butane if its heat of vaporization is 21.3 kJ/mol? | ΑΣφ ? Q= KJ You have already submitted this answer. Enter a new answer. No credit lost. Try again. Submit Previous Answers Request Answer Part F What volume does this much butane occupy at 760 torr and 37 °C? Η ΑΣΦ ? V= Submit Request Answer
How much heat is required to vaporize 100.0 g of ethanol, C2H,OH, at its boiling point? The enthalpy of vaporization of ethanol at its boiling point is 38.6 kJ/mol.
5) How much more heat is required to vaporize 48.7 g of ethanol (C,H,OH) than to vaporize 48.7 g of dichloromethane (CH2Cl2) ethanol dichloromethane AHvap is 40.5 kJ/mol AHvap is 31.6 kJ/mol AHfus is 5.02 kJ/mol AHfus is 6.20 kJ/mol Cs=2.46 J/gºC Cs= 1.19 J/g°C
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
How much heat energy is required to convert 15.0 g of solid ethanol at -114.5 °C to gasesous ethanol at 143.1 °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. How much heat energy...