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17.104:
a) The three possible final states are ice at a temperature below
C,
0
.
0
°
an ice-
water mixture at
C
0
.
0
°
or water at a temperature above
C.
0
.
0
°
To make an educated
guess at the final possibility, note that
)
C
K)(15.0
kg
J
kg)(2100
140
.
0
(
°
⋅
kJ
4.41
=
are
needed to heat the ice to
C,
0
.
0
°
and
)
C
K)(35.0
kg
J
kg)(4190
(0.190
°
⋅
kJ
27.9
=
must
removed to cool the water to
C,
0
.
0
°
so the water will not freeze. Melting all of the ice
would require an additional
kJ,
46.8
kg)
J
10
kg)(334
140
.
0
(
3
=
×
so some of the ice
melts but not all; the final temperature of the system is

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**Unformatted text preview: **C. . ° Considering the other possibilities would lead to contradictions, as either water at a temperature below freezing or ice at a temperature above freezing. b) The ice will absorb 27.9 kJ of heat energy to cool the water to C. ° Then, 070 . kg J 10 334 ) kJ 41 . 4 kJ 9 . 27 ( 3 = = ×-m kg will be converted to water. There will be 0.070 kg of ice and 0.260 kg of water....

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