How much heat energy, in kilojoules, is required to convert 34.0g of ice at −18.0 ∘C to water at 25.0 ∘C ? Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion: ΔHfus=334 J/g
Enthalpy of vaporization: ΔHvap=2250 J/g

Question

How much heat energy, in kilojoules, is required to convert 34.0g of ice at −18.0 ∘C to water at 25.0 ∘C ?  Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion: ΔHfus=334 J/g
Enthalpy of vaporization: ΔHvap=2250 J/g

aaronq · Answer

you have to do this in 3 steps and all all the q's together.
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aaronq · Answer

and add all*

anonymous · Answer

ok thanks so much

aaronq · Answer

no problem, if you're stuck just ask again.

anonymous · Answer

so  for the first part  q=mCdT  is it (34.0g * 2.09 J(g*C)*delta 43)?

aaronq · Answer

not quite, in the first part you're only going from -18 to 0 celsius

anonymous · Answer

ok so q= 1279.08 delta T would be +?

aaronq · Answer

$T_f-T_i=0-(-18)=18$ so yes, positive.

ookawaiioo · Answer

aaronq you are a beast