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physgrl
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Homework Statement
Suppose that 1 kg of water, initially at 350 K, is turned into steam at 373 K. What is the change in entropy? (Lv = 2.26 x 106 J/kg; cwater = 4186 J/(kg Co)
a. 6060 J/K
b. 6070 J/K
c. 6320 J/K
d. 6330 J/K
Homework Equations
ΔS=ΔQ/T
Q=mcΔT
Q=mL
The Attempt at a Solution
heat is needed to get the water to the boiling point 100C or 373K and then heat is needed
to vaporize the water
ΔS=(mcΔT+mL)/T
ΔS=(1kg*4186J/kg*23K+1kg*2.26x10^6)/373
ΔS=6320
and the answer key says it is supposed to be 6070
what am I doing wrong?