Question

during a science experiment, a student notices that when they burn a small amount of fuel in a closed container, the total energy of the system does not disappear but transforms into heat and light. they also observe that some heat spreads into the surrounding air, making the room warmer, and that the energy cannot be fully recovered to do work. which statement correctly applies the first and second laws of thermodynamics in this situation? the first law is violated because energy is lost, and the second law does not apply the first law is supported because energy disappears, and the second is violated because heat can be fully recovered. the first law is supported because energy is conserved, and the second law is supported because some energy spreads and cannot be fully recovered. both laws are violated because energy is transformed.

Explanation:

1. Recall the first law of thermodynamics: Energy is conserved (neither created nor destroyed, only transformed). In the experiment, energy transforms into heat and light, so energy is conserved—supporting the first law.
2. Recall the second law of thermodynamics: Energy tends to spread (increase in entropy), and not all energy can be fully recovered to do work. The experiment notes heat spreads and energy can’t be fully recovered—supporting the second law.
3. Analyze each option:

• First option: First law is not violated (energy is transformed, not lost), and second law does apply. Eliminate.
• Second option: First law says energy doesn’t disappear, and second law says heat can’t be fully recovered. Eliminate.
• Third option: Matches the first (energy conserved) and second (energy spreads, not fully recoverable) laws.
• Fourth option: Energy transformation is what the first law allows, so laws aren’t violated. Eliminate.

Answer:

The first law is supported because energy is conserved, and the second law is supported because some energy spreads and cannot be fully recovered.