The mass of the ice cube is 17.6 g, and its initial temperature is -11.9 °C. The water resulting from the melted ice reaches the temperature of your skin, 29.9 °C. How much heat is absorbed by the ice cube and resulting water?

Question

aaronq · Answer

you have to do this in a 3 step process, using equations:

(1) $q=H_{fusion}*m$
(2) $q=m*C_p*\Delta T$

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Region A: heating up the ice from -11.9 to 0 degrees, use equation (2), and appropriate specific heat capacity.

Region B: melting the ice (to water), use equation (1).

Region C: heating up the water, use equation (2), use appropriate specific heat capacity.

anonymous · Answer

afterwards do you add the q values together, right?

aaronq · Answer

oh yes ! sorry, i forgot to mention that lol

anonymous · Answer

this is what i did
Region A: (17.6)*(2.087)*(11.9)=437.101
Region B: I'm actually not sure but it says the enthalpy of fusion is 6010 j/mol and this is @ 1 mol
Region C: (17.6)(4.184)*(29.9)=2199.68
and add the J
Is this right?

aaronq · Answer

yeah thats right. for B since $H_{fusion}$ is given in moles you have to convert the mass to moles.

so (1) should be $q=H_{fusion}*n$

anonymous · Answer

okay cool thanks a lot! this helped

aaronq · Answer

no problem ! glad it did