1. An ice cube weighing 18g is removed from a freezer, where it has been at -20oC.
a. How much heat is required to warm it to 0oC without melting it?
b. How much additional heat is required to melt it to liquid water at 0 oC?
c. Suppose the ice cube was placed initially in a 180 g sample of liquid water at +20 oC in an insulated (thermally isolated) container. Describe the final state when the system has reached equilibrium.
334J/g Heat of Fusion
2260J/g Heat of Vaporization
2.1J/g°c Heat capacity of solid water
4.18J/g°c Heat capacity liquid water
a. How much heat is required to warm it to 0oC without melting it?
q=mCΔT
q=heat energy gained or lost by a substance
m=mass (grams)
C=specific heat
ΔT=change in temperature
Q= 18 x 2.1 x (20) = 756 J is required
b. How much additional heat is required to melt it to liquid water at 0 oC?
Q = 756 + 18 x 334 J = 6768J is required
c. Suppose the ice cube was placed initially in a 180 g sample of liquid water at +20 oC in an insulated (thermally isolated) container. Describe the final state when the system has reached equilibrium.
6768 = 180 x 4,18 (20-Tf)
8.99 = (20-Tf)
Tf = 20-8.99 = 110C
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