What quantity of heat is required to convert 50 g of ethanol (C2HsOH) at 23.0°C to...
Determine the amount of heat required to convert 500.0 g of liquid ethanol at 25.0°C into gaseous ethanol at 125°C. Use the following information on ethanol (C2H5OH) to calculate the amount of heat for each of the steps. Melting Point = −117°C Boiling Point = 78.3°C Molar Heat Capacities: Csolid =113 J/mol °C Cliquid = 420 J/mol °C ΔHfusion = 5.02 kJ/molΔHvaporization = 39.3 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...
How much heat (in kJ) is required to raise the temperature of 141,4 g of ethanol (mw=46,07) from 49.82 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat=2.46 J/gºC, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 288.7 g of ethanol (mw=46.07) from 39.38 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 202.8 g of ethanol (mw=46.07) from 40.34 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)
How much heat (in kJ) is required to raise the temperature of 124.9 g of ethanol (mw=46.07) from 30.24 °C to its boiling point of 78.37 °C and then vaporize it completely creating ethanol gas at the boiling temperature? (specific heat = 2.46 J/g°C, ΔHvap = 48.6 kJ/mol)
rams of ethanol (C2HSOH) from-120.0 C to 85.0 4. How much energy is needed to convert 25.0 g °C? 25 points molar heat capacity (solid) = 1 1 1 .46 J/mol*K molar heat capacity(liquid) 112.4 J/mol*K molar heat capacity(gas)- 78.28 J/mol*K heat of fusion 4.9 KJ/mol heat of vaporization = 38.56 KJ/mol melting point--114.1 C boiling point-783 C
How much heat energy is required to convert 16.2 g of solid ethanol at -114.5 °C to gasesous ethanol at 191.9 °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 is required to convert 55.6 g of solid ethanol at -114.5 °C to gasesous ethanol at 165.9 °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.
Given the following information for an unknown chemical: Specific heat (c) of solid phase: 1.75 J/g°C Heat of fusion (ΔHfus): 32.0 kJ/mol Specific heat (c) of liquid phase: 4.50 J/g°C Heat of vaporization (ΔHvap): 400. kJ/mol Specific heat (c) of vapor phase: 1.50 J/g°C Molar mass: 72.5 g/mol Freezing point: -15.00°C Boiling point: 15.00°C 1.Calculate the total energy needed (in kJ) to convert 15.5g of this chemical from -21.5°C to room temperature (23.0°C).