How does a balanced chemical equation demonstrate the law of conservation of mass?
A balanced chemical equation demonstrates the law of conservation of mass by showing that the total mass of the reactants equals the total mass of the products. This means that during a chemical reaction, the total number of atoms of each element remains constant.
In a balanced chemical equation, the coefficients in front of each compound represent the number of molecules or moles of that compound. These coefficients determine the ratio in which substances react and are formed.
According to the law of conservation of mass, matter cannot be created or destroyed during a chemical reaction. The total mass of the reactants before the reaction must equal the total mass of the products after the reaction. By balancing the chemical equation, it ensures that the number of atoms of each element on both sides of the equation is the same.
For example, in the reaction 2H2 + O2 → 2H2O, there are 4 hydrogen atoms and 2 oxygen atoms on the reactant side, and 4 hydrogen atoms and 2 oxygen atoms on the product side. The number of atoms is conserved, demonstrating the law of conservation of mass.
A balanced chemical equation demonstrates the law of conservation of mass by showing that the total mass of the reactants is equal to the total mass of the products. This law states that mass cannot be created or destroyed in a chemical reaction, but only transferred or rearranged.
In a chemical equation, the reactants are written on the left side and the products on the right side. The number of atoms of each element and the total mass on both sides of the equation must be equal.
For example, let's consider the reaction between hydrogen (H₂) and oxygen (O₂) to produce water (H₂O). The unbalanced equation is:
H₂ + O₂ → H₂O
To balance this equation, we need to ensure that the number of atoms of each element is the same on both sides. We can do this by adding coefficients in front of each compound:
2H₂ + O₂ → 2H₂O
By balancing the equation, we see that we have 4 hydrogen atoms and 2 oxygen atoms on both sides. The total mass of the reactants (2 * 2 g H₂ + 2 * 16 g O₂ = 4 g H₂ + 32 g O₂) is equal to the total mass of the products (2 * 18 g H₂O = 36 g H₂O). Therefore, the law of conservation of mass is upheld.
Balancing the chemical equation ensures that the number of atoms is conserved during the reaction, meaning that no atoms are lost or gained. This demonstrates that mass is conserved, even though the arrangement and bonding of atoms may change.
A balanced chemical equation demonstrates the law of conservation of mass by showing that the total mass of the reactants is equal to the total mass of the products.
To understand how a chemical equation demonstrates this law, let's take a look at an example. Consider the reaction between hydrogen gas (H2) and oxygen gas (O2) to form water (H2O).
The unbalanced equation for this reaction is:
H2 + O2 -> H2O
To balance this equation, we need to ensure that the same number of atoms of each element are present on both sides. We can achieve this by adjusting the coefficients in front of each molecule.
By balancing the equation, it becomes:
2H2 + O2 -> 2H2O
Now, let's analyze the mass of the reactants and products.
On the left-hand side of the equation, we have two molecules of hydrogen gas (H2) weighing 2(units) x 2(g per unit) = 4 grams, and one molecule of oxygen gas (O2) weighing 1(unit) x 32(g per unit) = 32 grams. The total mass of the reactants is 4 + 32 = 36 grams.
On the right-hand side of the equation, we have two molecules of water (H2O) weighing 2(units) x 18(g per unit) = 36 grams.
As we can see, the total mass of the reactants (36 grams) is equal to the total mass of the products (36 grams). This demonstrates the law of conservation of mass, which states that in a closed system, mass is neither created nor destroyed during a chemical reaction but only transformed from one form to another.
In summary, balancing a chemical equation ensures that the number of atoms of each element is the same on both sides and, consequently, the total mass remains conserved, proving the law of conservation of mass.