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Hypothetical Correlation Between Space, Potential Energy, and Conservation Laws in Chemical Reactions

Abstract

This paper explores a new hypothesis on how intra-atomic and inter-atomic space influences chemical reactions, specifically focusing on conservation of mass and conservation of energy laws. Using the example of the exothermic reaction between magnesium (Mg) and oxygen (O₂), we analyze how changes in density, inter-atomic space, and potential energy contribute to energy release. We also extend the discussion to an endothermic reaction (thermal decomposition of calcium carbonate, CaCO₃) to show the universality of the concept. The hypothesis suggests that while mass remains conserved, it is the manipulation of space within matter that governs energy transformations.

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Introduction

The classical conservation laws state:

Conservation of Mass: Mass can neither be created nor destroyed in chemical reactions.

Conservation of Energy: Energy can neither be created nor destroyed, only transformed.

However, experimental observations in exothermic and endothermic reactions show that reactants and products differ in density and potential energy. This raises the question: From where does the additional energy emerge or vanish? We propose that the answer lies in space transformations within matter, rather than changes in mass.

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Theoretical Background

1. Space as Energy

Intra-atomic space (within nucleus): regulates nuclear energy.

Inter-atomic space (between atoms): regulates potential energy and bond strength.

Space fluctuations lead to rearrangements in energy without altering mass.

2. Exothermic Example: Magnesium Burning in Oxygen

Balanced equation: 

Mass of Reactants: 48.6 g (Mg) + 32 g (O₂) = 80.6 g

Mass of Product: 80.6 g (MgO)

➡ Mass is conserved.

Enthalpy Change (ΔH): ≈ -1203 kJ/mol (exothermic release)

Density Change:

Mg: 1.74 g/cm³

O₂: 0.00143 g/cm³

MgO: 3.58 g/cm³

➡ Inter-atomic space decreases, density increases, potential energy drops, releasing heat.

3. Endothermic Example: Thermal Decomposition of CaCO₃

Balanced equation: 

Mass of Reactant: 100 g (CaCO₃)

Mass of Products: 56 g (CaO) + 44 g (CO₂) = 100 g

➡ Mass is conserved.

Enthalpy Change (ΔH): ≈ +178 kJ/mol (heat absorbed)

Density Change:

CaCO₃: 2.71 g/cm³

CaO: 3.34 g/cm³

CO₂: 0.00198 g/cm³

➡ Space within structure expands, potential energy rises, requiring absorption of heat.

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Graphical Representation

1. Potential Energy vs. Density Graph

Exothermic reactions: density ↑, potential energy ↓, heat released.

Endothermic reactions: density ↓ (overall system), potential energy ↑, heat absorbed.

2. Space Transformation Diagram

Reactants: higher inter-atomic space, less dense, higher potential energy.

Products: lower inter-atomic space (exothermic) or higher inter-atomic space (endothermic).

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Discussion

This hypothesis provides a new lens to interpret conservation laws:

Mass Conservation: Holds true universally, as atoms are neither created nor destroyed.

Energy Conservation: Apparent imbalance between reactant heat absorption and product heat release is explained by changes in inter-atomic and intra-atomic space.

Space as Regulator: Space is not mass, but it governs how potential energy transforms.

Thus, energy in reactions does not come from mass directly, but from the rearrangement of space within matter.

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Conclusion

We propose that:

1. Mass is conserved in all chemical reactions.

2. Energy transformations are driven by changes in inter-atomic and intra-atomic space.

3. Exothermic reactions compress space (higher density), releasing energy.

4. Endothermic reactions expand space (lower density), absorbing energy.

This view introduces space as the regulator of energy conservation, providing a new perspective for atomic and molecular physics.

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References

1. Atkins, P., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.

2. Cotton, F. A., & Wilkinson, G. (1999). Advanced Inorganic Chemistry. Wiley.

3. Levine, I. N. (2014). Quantum Chemistry. Pearson.

4. Experimental thermodynamic data: NIST Chemistry WebBook.