1. How much heat does it take to raise 50.0 g of liquid water to 120 °C if its initial temperature is 50 °C? (Possibly useful values: CH2O, liq = 4.184 J/g*°C, Csteam = 1.99 J/g*°C, Cice = 2.108 J/g*°C, ΔHfus = 6.01 kJ/mol, ΔHvap = 40.79 kJ/mol)
2. How much heat does it take to raise 50.0 g of liquid water to 50 °C if its initial temperature is -50 °C? (Possibly useful values: CH2O, liq = 4.184 J/g*°C, Csteam = 1.99 J/g*°C, Cice = 2.108 J/g*°C, ΔHfus = 6.01 kJ/mol, ΔHvap = 40.79 kJ/mol)
1. How much heat does it take to raise 50.0 g of liquid water to 120...
Use the following for all problems involving water: Cice = 2.09 J/gºC Cwater = 4.184 J/gºC Csteam = 2.03 J/gºC ΔHfus = 6.01 kJ/mol ΔHvap = 40.7 kJ/mol Question 1 (1 point) How many grams of ice at 0ºC can be melted by 7.70 kJ of heat? grams (3 SF) Blank 1:
Heat of fusion (ΔHfus) is used for calculations involving a phase change between solid and liquid, with no temperature change. For H2O, ΔHfus=6.02 kJ/mol. Specific heat capacity (C) is used for calculations that involve a temperature change, but no phase change. For liquid water, C=4.184 J/(g⋅∘C). Heat of vaporization (ΔHvap) is used for calculations involving a phase change between liquid and gas, with no temperature change. For H2O, ΔHvap=40.7 kJ/mol. How much heat is required to boil 77.5 g of...
Enter your answer in the provided box. How much heat (in kJ) is needed to convert 916 g of ice at -10.0°C to steam at 126.0°C? (The specific heats of ice, water, and steam are 2.03 J/g . oC, 4.184 J/g . oC, and 1.99 J/g , oC, respectively. The heat of fusion of water is 6.01 kJ/mol, the heat of vaporization is 40.79 k.J/mol.) k.J
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.)
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0C to water vapor at 182C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g C, and for steam is 1.99 J/g C. (Assume that the specific heat values do not change over the range of temperatures in the problem.)
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0°C to water vapor at 172°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g ·°C, and for steam is 1.99 J/g ·°C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) = KJ
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 (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)