How much heat is required to convert 155g of ice at -10°C into water vapor at 110°C?
sice = 2.09J/g·°C, swater = 4.18J/g·°C, svapor = 1.84J/g·°C, ΔHfusion = 6.01kJ/mol, ΔHvap = 40.67kJ/mol
How much heat is required to convert 155g of ice at -10°C into water vapor at...
The constants for H2O are shown here: Specific heat of ice: sice=2.09 J/(g⋅∘C) Specific heat of liquid water: swater=4.18 J/(g⋅∘C) Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250 J/g Part A How much heat energy, in kilojoules, is required to convert 73.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. 6.56 kJ is incorrect.
How much heat required to convert 36 grams (2 moles) of ice at 0 degrees C to liquid water at 50 degrees C? delta-H of fusion for H2O is 6.02 kJ/mol and the heat capacity of liquid water is 4.18J/g degrees C. A) 12 kJ B) 7524 J C) 8728 J D) 19564 J
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
How much heat is required to convert 5.0 kg of ice from a temperature of -10 C to water vapor at a temperature of 213 degrees F?
How much heat would be required to convert 173.3 g of ice to water at 0°C? (AHfus = 6.01 kJ/mol for water) 7 8 +/- x 100
6. How much heat energy is required to convert 250 g of ice at - 25° C to steam at 110°C ? Sp. Heat capacity of ice = 2.1 X103T/kgºc Sp. Heat capacity of water = 4.2X10 J/kg °C Sp. Heat capacity of steam = 2.0X102/kg 0 C Latent heat of fusion = 3.3X105J/kg Latent heat of vapourization = 2.3X106J/kg [T 10]
Calculate the heat required in Joules to convert 18.0 grams of water ice at a temperature of -20° C to liquid water at the normal boiling point of water. Given: -specific heat of ice = 2.09 J/g°C -specific heat of liquid water = 4.184 J/g°C -specific heat of water vapor = 2.03 J/g°C -molar heat of fusion of water = 6.02 kJ/mol -molar heat of vaporization of water = 40.7 kJ/mol
How much energy (in kilojoules) is released when 31.5 g of ethanol vapor at 97.0 ∘C is cooled to -13.5 ∘C? Ethanol has mp = -114.5 ∘C, bp = 78.4 ∘C, ΔHvap = 38.56 kJ/mol and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K⋅mol) for the liquid and 65.7 J/(K⋅mol) for the vapor.
5) How much heat is required to convert 0.05kg of water at 298 K to super-steam at 423 K. The boiling point of water is 373 K. Cm [H2O (l)] = 75.4 J/(mol. ℃) Cm [H2O (g)] = 33.6 J/(mol. ℃) ΔHvap = 40.67 75.4 J/mol
calculate the amount of heat in KJ that is required to heat 25.0g of ice from -25c to 105degrees celciusto 105 degrees celcius in a close vessel and sketch a heating curve for the process.The specific heat of ice is 2.11J/(g.degrees celcius);4.18J/(g.degrees celcius for water2.00J/g.degrees celcius.DH for water is 6.01KJ/mol;DH for water 40.67KJ/mol