How much heat is required to vaporize 30.8 g of water at 100 ∘C∘C? (ΔHvap(H2O)=40.7kJ/mol, Heat capacity(H2O)=4.184J/g∘C)(ΔHvap(H2O)=40.7kJ/mol, Heat capacity(H2O)=4.184J/g∘C) Express your answer with the appropriate units.
At 1 atm, how much energy is required to heat 75.0 g H2O(s) at -14.0°C to H2O(g) at 119.0 °C? Use the heat transfer constants found in this table.
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 is required to vaporize 37.3 gg of water at 100 ∘C∘C? (ΔHvap(H2O)=40.7kJ/mol,Heatcapacity(H2O)=4.184J/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.)
How much heat (in kJ) is required to convert 431 g of liquid H2O at 24.0°C into steam at 157°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.
At 1 atm, how much energy is required to heat 75.0 g H2O(s) at −22.0 ∘C to H2O(g) at 147.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 73.0 g H2O(s) at −14.0 ∘C to H2O(g) at 123.0 ∘C? Use the heat transfer constants found in this table.
At 1 atm, how much energy is required to heat 73.0 g H2O(s)73.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 159.0 ∘C?159.0 ∘C? Use the heat transfer constants found in this table. Heat-transfer constants for H2O at 1 atm Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C)...
At 1 atm, how much energy is required to heat 43.0 g H2O(s)43.0 g H2O(s) at −14.0 ∘C−14.0 ∘C to H2O(g)H2O(g) at 121.0 ∘C?121.0 ∘C? Use the heat transfer constants found in this table. Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O...