Why does steam at 100°C cause more severe burns than boiling water at 100°C?

This is a very popular question in competitive exams related to latent heat. Option A (Steam has higher temperature than water) is incorrect — both steam and boiling water are at the same temperature: 100°C (at standard atmospheric pressure). There is no temperature difference between them. If the temperature were higher for steam, the question would be trivial and uninteresting. Option B (Steam contains more latent heat which it releases on condensing) is CORRECT — the image states: 100°C की भाप द्वारा उत्पन्न जलन 100°C के पानी की अपेक्षा अधिक गंभीर होती है क्योंकि भाप में गुप्त ऊष्मा अधिक होती है। When steam at 100°C touches the skin, it first condenses to water at 100°C, releasing the latent heat of vaporization (540 cal/g = 2260 J/g). This additional energy is transferred to the skin, causing more severe burns than boiling water at the same temperature. Boiling water only transfers its sensible heat as it cools. Option C (Steam is lighter and spreads more quickly) is incorrect — the spreading of steam has no direct relation to the severity of burns in this context. The physics explanation is entirely based on latent heat. Option D (Steam has higher pressure than boiling water) is incorrect — at 100°C and 1 atm, steam pressure equals atmospheric pressure. Steam in this context is not under