# What is the specific heat of ice

## Internal energy - heat capacity

#### Preliminary remark

If you take a piece of ice out of the freezer and put it in a warm place, it will start to melt. This means that water in solid form changes into water in liquid form. To do this, the water molecules have to be converted from the relatively firm bond in the ice into the weaker bond that exists between water molecules in the liquid state, using energy. Breaking the solid bonds requires energy, which the melting ice draws from its warmer surroundings.

Melting ice - like its surrounding meltwater - has a temperature ϑ = 0 ° C. The transformation from solid ice to liquid takes place without Temperature change.

#### Aim of the experiment

First of all, the melting energy \ (E _ {\ rm {s}} \) for a certain piece of ice should be determined (body size). Then the specific heat of fusion (material size) \ (s = \ frac {E _ {\ rm {s}}} {m _ {\ rm e}} \) is determined from this.

#### Carrying out the experiment

• The ice removed from the freezer is left in the air for a while until the surface melts (we want to use ice at 0 ° C).
• Water is filled into the calorimeter vessel (mw, ϑw, cw)
• On the scales with which the ice is weighed, we first place a filter paper and then the piece of ice. We weigh ice and filter paper (m2), dry the ice well and then put it in the calorimeter container. The moist filter paper still on the scales has the mass m1. The following applies to the mass of the ice: \ (m_ {rm e} = m_2-m_1 \)
• The calorimeter water is stirred until the ice has completely melted and a temperature minimum ϑm has set.