- #1
physgirl
- 99
- 0
so there're:
0.041 kg ice cube at 0.0 *C
0.110 kg water at 40.0 *C
in
0.062 kg iron cup at 40.0 *C
Find the equilibrium temperature of the cup and its contents:
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So what I tried doing was... I found the heat lost by water if cooled to 0 *C, which was 18418.4 J (mass of water * water specific heat * temperature difference which is 40)
then found th eheat needed to melt ice, which was 13735 J (mass of ice * Lf)
then found the difference of the two to find the amount of heat left... and used that much heat to warm 0.151 kg of water (mass of initial water + initial ice) at 0 *C to its final temperature... so I did, delta T=Q/(mc) which gave T=7.4 *C...
so then I used that temperature in kelvin, which is 280.6 K and did:
(specific heat of water)(mass of water which is now 0.151)(280.6+T)=(specific heat of iron)(mass of cup)(313-T)
and solved for T... where did I make the mistake because this answer's not correct?
0.041 kg ice cube at 0.0 *C
0.110 kg water at 40.0 *C
in
0.062 kg iron cup at 40.0 *C
Find the equilibrium temperature of the cup and its contents:
-------
So what I tried doing was... I found the heat lost by water if cooled to 0 *C, which was 18418.4 J (mass of water * water specific heat * temperature difference which is 40)
then found th eheat needed to melt ice, which was 13735 J (mass of ice * Lf)
then found the difference of the two to find the amount of heat left... and used that much heat to warm 0.151 kg of water (mass of initial water + initial ice) at 0 *C to its final temperature... so I did, delta T=Q/(mc) which gave T=7.4 *C...
so then I used that temperature in kelvin, which is 280.6 K and did:
(specific heat of water)(mass of water which is now 0.151)(280.6+T)=(specific heat of iron)(mass of cup)(313-T)
and solved for T... where did I make the mistake because this answer's not correct?