What is the total energy transfer(in KJ) when 10.00 pounds of water vapor at 110 degrees C becomes ice at 253K? Assume that the specific gravity of water = 1.00.
Convert 10.00 pounds H2O to grams.
q1 = mass H2O x specific heat steam x (110=100)
q2 = mass H2O x heat vaporization
q3 = mass H2O x specific heat liquid water x (100-0)
q4 = mass water x heat fusion.
Total Q = sum of individual q values.
In q1, did you mean to say (110-100)? I did it assuming that and after I added all the q values I got 13,759.78 KJ as my answer. Is that correct?
Also shouldn't there be another phase involving the Cs of ice where the ice is cooled down to the 253k?
To calculate the total energy transfer in kilojoules (KJ) when 10.00 pounds of water vapor at 110 degrees Celsius becomes ice at 253K, we need to consider the energy required for each phase change.
First, let's convert the given weight from pounds to kilograms since the standard unit for measuring energy is in joules, which is based on the metric system.
1 pound is approximately 0.4536 kilograms.
10.00 pounds * 0.4536 kilograms/pound = 4.536 kilograms
Next, we need to calculate the energy required to cool the water vapor from 110 degrees Celsius to 0 degrees Celsius. The specific heat capacity of water vapor is 2.03 J/g°C.
To convert this to joules, we need to multiply by the mass (in grams) and the change in temperature:
Energy = specific heat capacity * mass * change in temperature
Change in temperature = final temperature - initial temperature
Change in temperature = 0°C - 110°C = -110°C
We need to convert this temperature change to Kelvin:
Change in temperature = -110 + 273 = 163K
Energy = 2.03 J/g°C * 4536g * 163°C = XXXXXXX joules
Next, we need to calculate the energy required for the phase change from water vapor to liquid water. The heat of vaporization for water is 40.7 kJ/mol. The molar mass of water is 18.02 g/mol.
To calculate the moles of water, we divide the mass by the molar mass:
Moles = mass / molar mass
Moles = 4536g / 18.02 g/mol = XXXXXXX moles
The energy required for the phase change from vapor to liquid is calculated using the equation:
Energy = heat of vaporization * moles
Energy = 40.7 kJ/mol * XXXXXXX moles = XXXXXXX kJ
Lastly, we need to calculate the energy required for the phase change from liquid water at 0 degrees Celsius to ice at 253K. The specific heat capacity of ice is 2.09 J/g°C.
Using the same equation as before:
Energy = specific heat capacity * mass * change in temperature
Change in temperature = final temperature - initial temperature
Change in temperature = 253K - 0°C = 253K
Energy = 2.09 J/g°C * 4536g * 253°C = XXXXXXX joules
Summing up these three values will give us the total energy transfer in kilojoules.