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)
How much heat (in kJ) is required to raise the temperature of 124.9 g of ethanol...
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 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)
QUESTION 3 How much heat (in kJ) is required to raise the temperature of 122 g of ethanol (mw 46.07) from 11.29 °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, AHyap = 48.6 kJ/mol) QUESTION 4 What is the change in enthalpy (in kJ) when 40.1 g of ethanol (mw-46.07) is condensed at its boiling temperature? (specific heat 2.46 J/g°C, AHvap 48.6 kJ/mol)...
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
Calculate the amount of heat (in kJ) required to raise the temperature of 14.0 g of liquid H_2O (molar mass = 18.0 g/mol) from 25.0 degree C to the boiling point and then to vaporize the liquid at that temperature, (specific heal capacities: H_2O(s): 2.06 J/g degree C, H_2O(l): 4.18 J/g degree C, H_2O(g): 1.92 J/g degree C; heat of fusion of H_2O: 6.02 kJ/mol; heat of vaporization of H_2O: 40.7 kJ/mol; melting point of H_2O: 0.0 degree C, boiling...
What quantity of heat is required to convert 50 g of ethanol (C2HsOH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat of ethanol = 2.46 J/g·C; ΔHvap-39.3 kJ/mol) A) 42.7 kJ B) 49.5 kJ C) 159 kJ D) 1970 k.J E) 6840 kJ
Determine the amount of heat energy (in kJ) needed to warm a 58.5-g sample of ethanol (C2H5OH) from-150°C to 55°C. C2H5OH 46.07 g/mol AHvap 38.56 kJ/mol ΔΗrus 4.90 kJ/mol Boiling Point 78.5°C Freezing Point -117.3°C Specific Heat Capacity (c) of solid 0.249 J/g.°C Specific Heat Capacity (c) of liquid 2.44 J/g.°C Specific Heat Capacity (c) of gas 1.70 J/8.°C
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
How much heat (in kJ) is required to convert 431 g of liquid H2O at 23.6°C into steam at 148°C? (Assume that the specific heat of liquid water is 4.184 J/g·°C, the specific heat of steam is 2.078 J/g·°C, and that both values are constant over the given temperature ranges. The normal boiling point of H2O is 100.0°C. The heat of vaporization (ΔHvap) is 40.65 kJ/mol.)