2.26 g of liquid water at 23.5 ◦c was com- pletely converted to ice at 0 ◦c. how much heat was (absorbed/released) by the system during this process?

Givens

m = 2.26 g

c = 4.19 J/(g * oC)

Δt = 23.5oC - 0 = 23.5oC

hf = heat of fusion for ice = 334 J/g

Equation

H = m*c*Δt +  hf * m

H = m*(c*Δt + hf)

Solution

H = 2.26 * (4.19 * 23.5  + 334)

H = 2.26 * (432.5)

H = 977.4 J

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16

explanation:

the marks go by 4s