How Much Energy Is Needed to Convert 500 g of Water at 20°C to Steam at 100°C?

AI Thread Summary
To convert 500 g of water at 20°C to steam at 100°C, two steps are required: heating the water to 100°C and then vaporizing it. The specific heat capacity of water is essential for calculating the energy needed to raise the temperature, while the latent heat of vaporization is used for the phase change from liquid to gas. The relevant equations include Eh = mct for heating and Eh = mLf for vaporization. It's important to note that "T" in the equations refers to the change in temperature, denoted by the delta symbol. Understanding these concepts is crucial for solving the problem effectively.
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Homework Statement



How much energy does it take to transform 500 g (0.5kg) of liquid water at 20 oC to steam at 100 oC? Note that the specific heat capacity of liquid water is 4.28x10^3 J/Kg/oC and the latent heat of vaporization for water is 2.3x10^6 J/Kg.

Homework Equations


Eh=mct ; m1c1t1=-m2c2t2 ; Eh = mLf ; Eh= mLv


The Attempt at a Solution



no clue..please help..
 
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Two steps. first the water needs to be heated to 100 C, then the water has to evaporate. Both steps involve heat going into the water. Which two of those 4 equations do you need?

By the way, in the first and second equation you list, it is not "T" but "change in T." (The triangle, "delta," means "change in...")
 

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