How much heat must be added to 65 g of water at an initial temperature of 54°C to completely convert the 100°C?
How much heat must be added to 65 g of water at an initial temperature of 54°C to completely convert the 100°C water to steam?
I calculated how much heat is needed for boiling point in this scenario but the same formula did not work for steam. Am I supposed to use a different formula?
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specific heat of water is 4.186 kJ/kgC
heat of vaporization of water is 2256 kJ/kg
energy needed to heat water to 100ºC
E1 = 4.186 kJ/kgC x 0.065 kg x (100–54)
energy needed to boil water
E2 = 2256 kJ/kg x 0.065 kg
add the two together for total.
To raise the temperature of water: m * c * delta-C where m = mass of water, c = specific heat of water and delta-T = change in temperature from 54 C to 100 C.
Then to convert to steam at 100 C takes energy m * c_latent where c_latent = latent heat of vaporization for water. The result is steam at 100 C.