anonymous
  • anonymous
Water's heat of fusion is 80. cal/g , and its specific heat is 1.0calg⋅∘C . Some velomobile seats have been designed to hold ice packs inside their cushions. If you started a ride with ice packs that held 1900g of frozen water at 0 ∘C , and the temperature of the water at the end of the ride was 32 ∘C , how many calories of heat energy were absorbed?
Physics
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SOLVED
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chestercat
  • chestercat
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aaronq
  • aaronq
Given: 1900g of frozen water at 0 ∘C (1900 g of ice) \(\Delta H_{fusion}=80\;cal/g\) ; \(C_p^{\;water}=1\;cal/g*^oC\) Find the heat req'd to melt the ice: \(q_{fusion}=\Delta H_{fusion}*m_{ice}\) Now, find the heat req'd to raise the temp of the water to -32 centigrade \(q_{water}=m_{water}*C_p^{\;water}*\Delta T\); where, \(\Delta T=T_f-T_i\) Add the heat of both to get the total heat absorbed: \(q_{total}=q_{fusion}+q_{water}\)
aaronq
  • aaronq
i meant 32 not "-32"

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