Week 4 Achieve 10

[Kaethe Zappacosta 2L]

An ice cube with a mass of 52.6 g at 0.0 ∘C is added to a glass containing 359 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, ΔH∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings


I found T final completely fine, but then the feedback told me that "the heat needed to melt the ice, ΔHfus , has not been accounted for. Calculate deltaHfus by multiplying the number of moles of ice by ΔH∘f . Then, factor this energy into the calculation.

Why do we need to do this, and why is delta Hfusion=-q(water)-q(ice)?

[Anna Wilborn-1L]

The ice first needs to melt to liquid before the temperature of then melted ice can rise.

q melted ice + delta Hfusion = - q water because water is the surrounding and the ice is the system

[Kathleen Wijaya 3L]

∆Hfusion is important because the ice will undergo a phase change as it melts in the warmer water; we need to take this into account because it takes energy to melt ice.

[305589333]

Ice will have to go through a phase change as the warm water causes it to melt which requires energy