How many kJ of energy are released when 96.0 g of water is converted to ice?
Water heat of fusion = 334 J/g
Water heat of vaporization = 2260 J/g

To calculate the energy released when 96.0 g of water is converted to ice, we use the formula:

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

Where:
- \( Q \) is the amount of heat energy released (in joules, J).
- \( m \) is the mass of water (in grams, g).
- \( \Delta H_f \) is the heat of fusion of water (334 J/g).

Now, let's calculate the energy:

\[
Q = 96.0 \, \text{g} \cdot 334 \, \text{J/g} = 32,064 \, \text{J}
\]

Convert joules to kilojoules:

\[
32,064 \, \text{J} \div 1000 = 32.064 \, \text{kJ}
\]

So, **32.064 kJ** of energy are released when 96.0 g of water is converted to ice.

Would you like further clarification or details?

### Related Questions:
1. What is the total energy required to melt 96.0 g of ice into water?
2. How much energy is required to vaporize 96.0 g of water?
3. How does the heat of fusion of other substances compare to water?
4. What is the role of latent heat in phase changes?
5. How does the heat of fusion vary with temperature and pressure?

### Tip:
Always convert energy units to match the question’s requirements (e.g., from joules to kilojoules or calories).

How many kJ of energy are released when 96.0 g of water is converted to ice? Water heat of fusion = 334 J/g Water heat of vaporization = 2260 J/g

Calculate the energy released when 96.0 g of water is converted to ice using the heat of fusion (334 J/g). Learn step-by-step how to apply the formula Q = m * ΔH_f and convert joules to kilojoules. This problem is suitable for high school students learning about thermodynamics and phase changes.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation