How many joules of energy is required to melt a five-pound (5.00 pounds, 1 pound = 454 g) bag of ice at 0°C? The latent heat of fusion of ice is 333 J/g.

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

\[
Q = m \times L_f
\]

Where:
- \( Q \) is the heat energy required (in joules),
- \( m \) is the mass of the ice (in grams),
- \( L_f \) is the latent heat of fusion of ice (in joules per gram).

### Step 1: Convert pounds to grams
Given:
- Mass of ice = 5.00 pounds
- 1 pound = 454 grams

So,
\[
m = 5.00 \, \text{pounds} \times 454 \, \text{grams/pound} = 2270 \, \text{grams}
\]

### Step 2: Calculate the energy required
Given:
- Latent heat of fusion \( L_f = 333 \, \text{J/g} \)

Now, calculate the energy \( Q \):
\[
Q = 2270 \, \text{grams} \times 333 \, \text{J/g} = 755910 \, \text{J}
\]

So, **755,910 joules** of energy is required to melt the 5-pound bag of ice at 0°C.

Would you like any further details or have any questions?

Here are 5 related questions:
1. How much energy is required to raise the temperature of the melted water from 0°C to 100°C?
2. What is the specific heat capacity of ice, and how does it compare to water?
3. How much time would it take to melt the ice if 100 watts of power is applied?
4. How would the energy required change if the ice started at a temperature below 0°C?
5. How does the latent heat of fusion compare to the latent heat of vaporization?

**Tip:** When calculating energy, always ensure units are consistent for accurate results.

Discover how to calculate the energy needed to melt a five-pound bag of ice at 0°C using the latent heat of fusion formula. Learn how to convert pounds to grams and apply the formula Q = m × Lf. This step-by-step solution is suitable for students in Grades 9-12.

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