- For the reaction \(2Na + Cl_2\), balancing the atoms results in \(2NaCl\).
- For the decomposition reaction \(2MgO\), breaking it into elemental constituents results in \(2Mg + O_2\).
- The identified products are \(\boxed{2NaCl}\) and \(\boxed{2Mg + O_2}\).
Explanation
- Analyzing the first reaction: 2Na + Cl_2
To predict the missing products in the given chemical reactions, we must adhere to the law of conservation of mass, which states that the number of atoms of each element must be equal on both sides of the reaction. We also consider the valency of the elements involved.
For the first reaction: \(2Na + Cl_2 \rightarrow ?\)
- On the left side, we have 2 Sodium (Na) atoms and 2 Chlorine (Cl) atoms (as \(Cl_2\) is a diatomic molecule).
- Sodium typically forms a \(+1\) ion (\(Na^+\)) and Chlorine forms a \(-1\) ion (\(Cl^-\)). Thus, they form the stable ionic compound Sodium Chloride (\(NaCl\)).
- To balance the 2 Na and 2 Cl atoms from the reactants, the product must be \(2NaCl\). Comparing this to our options, \(2NaCl\) is the correct product.
- Analyzing the second reaction: 2MgO
For the second reaction: \(2MgO \rightarrow ?\)
- This represents a decomposition reaction, where a compound breaks down into its constituent elements. Magnesium oxide (\(MgO\)) is composed of Magnesium (Mg) and Oxygen (O).
- Elemental Magnesium exists as \(Mg\), and elemental Oxygen exists as the diatomic gas \(O_2\).
- Looking at the reactants, we have 2 Magnesium atoms and 2 Oxygen atoms.
- Breaking these down, we get 2 Mg atoms and 1 molecule of \(O_2\).
- Thus, the balanced product is \(2Mg + O_2\). Comparing this to our options, \(2Mg + O_2\) is the correct product.
- Conclusion
By applying the law of conservation of mass and knowledge of chemical properties:
- For \(2Na + Cl_2 \rightarrow ?\), the balanced equation is \(2Na + Cl_2 \rightarrow 2NaCl\).
- For \(2MgO \rightarrow ?\), the balanced equation is \(2MgO \rightarrow 2Mg + O_2\).
Therefore, the missing components are \(2NaCl\) and \(2Mg + O_2\).
Examples
Chemical reactions are fundamental to everything from the metabolism in our bodies to the manufacturing of essential materials. For example, the reaction between sodium and chlorine is used to create table salt (NaCl), which is vital for human health. Similarly, the decomposition of metal oxides is a common process in metallurgy, where scientists extract pure metals like magnesium from their ores for use in lightweight alloys for cars and aircraft. Understanding these balanced equations helps chemists scale up industrial production efficiently and safely.