To tackle this question, we need to understand the concepts of latent heat and the processes involved in changing states of matter. Specifically, we are looking at the heat required to convert ice to water and the heat needed to convert boiling water to steam.
Latent Heat Explained
Latent heat is the amount of heat energy required to change the state of a substance without changing its temperature. There are two key types of latent heat relevant to this question:
- Latent Heat of Fusion: This is the heat required to convert a solid into a liquid at its melting point. For ice, this is the heat needed to turn it into water at 0°C.
- Latent Heat of Vaporization: This is the heat required to convert a liquid into a gas at its boiling point. For water, this is the heat needed to turn it into steam at 100°C.
Calculating Q1 and Q2
Let's denote:
- Q1 = Latent heat of fusion of ice (0°C to water at 0°C)
- Q2 = Latent heat of vaporization of water (100°C to steam at 100°C)
The values for these latent heats are approximately:
- Q1 (latent heat of fusion) ≈ 334 Joules per gram
- Q2 (latent heat of vaporization) ≈ 2260 Joules per gram
Comparing Q1 and Q2
Now, when we compare Q1 and Q2, we see that:
- Q1 (334 J) is significantly less than Q2 (2260 J).
This means that the heat required to convert boiling water to steam (Q2) is much greater than the heat required to convert ice to water (Q1).
Conclusion on the Comparison
Based on the values and the processes involved, we can conclude that:
Thus, the correct answer to your question is (B) Q2 > Q1. This illustrates the significant energy required to overcome the intermolecular forces when changing from liquid to gas compared to solid to liquid.
