Calculate the heat change in kilojoules for melting 8.00 kg of ice at 0 deg * C .

To calculate the heat change required to melt ice, we use the formula:

\[
q = m \cdot \Delta H_f
\]

where:
- \( q \) is the heat change in joules (J),
- \( m \) is the mass of the ice in kilograms (kg),
- \( \Delta H_f \) is the heat of fusion for ice.

The heat of fusion (\( \Delta H_f \)) for ice is **334 kJ/kg**.

Given:
- Mass of ice, \( m = 8.00 \) kg,
- Heat of fusion for ice, \( \Delta H_f = 334 \) kJ/kg.

### Calculation

\[
q = 8.00 \, \text{kg} \times 334 \, \text{kJ/kg} = 2672 \, \text{kJ}
\]

So, the heat change required to melt 8.00 kg of ice at 0°C is **2672 kJ**.

Would you like to know more details or have any questions?

Here are some related questions that might interest you:

1. How much energy is required to melt ice and then raise the temperature of the resulting water to 100°C?
2. What is the difference between the heat of fusion and heat of vaporization?
3. How does pressure affect the melting point of ice?
4. How much ice can be melted with 5000 kJ of energy?
5. What is specific heat capacity, and how is it different from heat of fusion?

**Tip:** When calculating heat changes, always ensure that the units of mass and energy are consistent.

Calculate the heat change in kilojoules for melting 8.00 kg of ice at 0°C.

Learn how to calculate the heat change required to melt 8.00 kg of ice at 0°C. This problem demonstrates thermodynamic principles, including the heat of fusion, and provides a step-by-step solution using the formula q = m ⋅ ΔH_f. Ideal for high school students in Grades 9-12.

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