How much heat energy is released when 50 grams of steam condenses into water at 100°C? (Latent heat of vaporization for water = 2260 J/g)

To calculate the heat energy released when 50 grams of steam condenses into water at 100°C, we can use the formula:

\[
Q = m \cdot L_v
\]

Where:
- \( Q \) is the heat energy released (in joules),
- \( m \) is the mass of the steam (in grams),
- \( L_v \) is the latent heat of vaporization (in J/g).

Given:
- \( m = 50 \, \text{g} \),
- \( L_v = 2260 \, \text{J/g} \).

Now substitute the values:

\[
Q = 50 \, \text{g} \cdot 2260 \, \text{J/g} = 113,000 \, \text{J}
\]

So, the heat energy released is **113,000 J** (or **113 kJ**).

Would you like to explore the process further or ask more about heat transfer concepts?

Here are 5 related questions for you to consider:
1. How much heat energy would be required to turn water at 100°C into steam?
2. What is the difference between latent heat of vaporization and latent heat of fusion?
3. How does the amount of heat released during condensation compare with freezing water?
4. How would the heat energy change if the mass of steam were different?
5. What is the total energy involved in heating water from 0°C to steam at 100°C?

**Tip:** Always check the state of the substance (solid, liquid, or gas) when calculating heat energy for phase changes!

Discover how to calculate the heat energy released when 50 grams of steam condenses into water at 100°C. Using the latent heat of vaporization (2260 J/g), this problem applies key thermodynamics concepts. Ideal for students in Grades 9-12.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation