contestada

A
14.7

g
ice cube is placed into
324

g
of water. Calculate the temperature change in the water upon complete melting of the ice. Hint: Determine how much heat is absorbed by the melting ice and then use
q
=
m
C
Δ
T
to calculate the temperature change. Use the heat of fusion for water to calculate "q"

Respuesta :

Answer:

[tex]\Delta T=3.615^{\circ}C[/tex] is the drop in the water temperature.

Explanation:

Given:

  • mass of ice, [tex]m_i=14.7\ g=0.0147\ kg[/tex]
  • mass of water, [tex]m_w=324\ g=0.324\ kg[/tex]

Assuming the initial temperature of the ice to be 0° C.

Apply the conservation of energy:

  • Heat absorbed by the ice for melting is equal to the heat lost from water to melt ice.

Now from the heat equation:

[tex]Q_i=Q_w[/tex]

[tex]m_i.L=m_w.c_w.\Delta T[/tex] ......................(1)

where:

[tex]L=[/tex] latent heat of fusion of ice [tex]=333.55\ J.g^{-1}[/tex]

[tex]c_w=[/tex] specific heat of water [tex]=4.186\ J.g^{-1}.^{\circ}C^{-1}[/tex]

[tex]\Delta T=[/tex] change in temperature

Putting values in eq. (1):

[tex]14.7 \times 333.55=324\times 4.186\times \Delta T[/tex]

[tex]\Delta T=3.615^{\circ}C[/tex] is the drop in the water temperature.

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