Final Answer:
The energy needed to melt 50 grams of 0°C ice is 16,700 joules. This energy is required to overcome the intermolecular bonds and transition the substance from a solid to a liquid state.
Step-by-step explanation:
To calculate the energy needed to melt 50 grams of 0°C ice, we can use the formula:
\[ Q = m \cdot L_f, \]
where \( Q \) is the heat energy, \( m \) is the mass of the substance, and \( L_f \) is the heat of fusion. For water, the heat of fusion (\( L_f \)) is approximately 334 J/g.
Substituting the values into the formula:
\[ Q = 50 \, \text{g} \cdot 334 \, \text{J/g} = 16,700 \, \text{J}. \]
Therefore, it would take 16,700 joules of energy to melt 50 grams of ice at 0°C.
To understand why this energy is needed, consider the process of phase change. At 0°C, the ice is in a solid state. To convert it into liquid water, energy must be supplied to break the intermolecular bonds holding the ice molecules together. This energy is used to overcome the forces of attraction between the molecules, allowing them to move more freely in the liquid state.
The heat of fusion represents the amount of energy required to change a substance from a solid to a liquid at its melting point. In the case of water, this is the energy needed to overcome the hydrogen bonds between water molecules in the solid state.
In summary, to melt 50 grams of 0°C ice, 16,700 joules of energy are needed to break the molecular bonds and transition the substance from a solid to a liquid state.