Introduction
The law of conservation of mass is a very important concept, it says that we cannot create or destroy the mass; however, this mass can be transformed into another form.
In Physics, we express the law of conservation of mass as the differential form by continuity equation of the mechanics of fluids and continuum mechanics with the following equation:
∂ρ/∂t +⛛(ρv) = 0
Where,
ρ = density
t = time
v = velocity
⛛ = divergence
The law of conservation of mass states that in all the physical and chemical processes, the total mass of products in a chemical reaction is equal to the mass of reactants.
What is the Law of Conservation of Mass?
The Law of conservation of mass was studied by a French Chemist named Antoine Lavoisier in 1789.
This law states that in a chemical reaction, the mass of products in chemical reactions equals the mass of reactants.
According to this law, the matter cannot be created nor be destroyed. We call this law the law of indestructibility of matter. Let’s study the following experiments as the law of conservation of mass examples to get clarity in the conservation of mass definition:
When Matter Undergoes a Physical Change
Take a piece of ice (ice is solid water) and place it in a conical flask. This flask is properly corked and weighted and it is now heated gently to melt the ice into water.
Ice → Heat → Water
(solid) (Liquid)
The flask is weighed again, we notice that the weight of the flask remains the same because the mass of ice does not change after it undergoes a physical change.
When Matter Undergoes a Chemical Change
A Swiss Chemist named Hans Heinrich Landolt took two test tubes joined with a common line as shown below:
(Image will be uploaded soon)
One tube contains a solution of sodium chloride and another contains a silver nitrate solution; the tube containing these two solutions is called Landolt’s tube.
Both tubes were corked and weighed. Now, the above arrangement is tilted to let these solutions mix. The chemical reaction occurs, resulting in a curdy white precipitate of silver chloride. The reaction is as follows:
Nacl (s) + AgNO3 (aqueous) → AgCl (s) + NaNO3 (aqueous)
Sodium chloride Silver Nitrate Silver Chloride Sodium Nitrate
(White precipitate)
After this reaction, the above arrangement was weighed again, it was found that the weight remains the same.
Decomposition of Mercuric Oxide (HgO)
When 100 g of HgO is heated, it decomposes into two compounds viz: one mole of Hg and a half mole of O2. The reaction occurs in the following manner:
HgO (s) → Hg (l) + ½ O2
Mercuric Oxide Mercury Oxygen
100 g 92.6 g 7.4 g
Here, if we calculate the mass of products viz: Hg and O2, i.e., 92.6 + 7.4 = 100g, which is equivalent to the mass of the reactant, i.e., HgO. So, the law of conservation of mass verifies here.
Combustion Process
When we burn pieces of wood, these pieces turn to ashes, water vapor, and carbon dioxide.
If we weigh the piece of wood and after burning it, ashes, water vapors, and CO2 are heated, there will not be any change in the mass before and after the reaction.
Now, let’s look at some more examples of the law of conservation of mass:
Law of Conservation of Mass Examples
Example 1:
Take a container and place 16 g of methane or CH4 and 64 g of O2. After the container is closed, CH4 and O2 remain closely packed. Now, ad the reaction proceeds, i.e., the combustion reaction, we get the following products:
CH4 (gas) + 2 O2 (g) → CO2 (g) + 2 H2 O (g)
Methane Oxygen Carbon Dioxide Water vapor
16 g 64 g 44 g
Here, before the reaction, the total mass of reactants was:
16 + 64 = 80 g
So, here what do you expect could be the mass of water vapor after the reaction?
Well, by the law of conservation of mass, the total mass of products must be 80 g.
44 + mass of H2O = 80 g.
So, we get the mass of 2 moles of H2O as 36 g.
Therefore, our final balanced equation after applying the principle of conservation of mass is:
CH4 (gas) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
Methane Oxygen Carbon Dioxide Water vapor
16 g 64 g 44 g 36 g
From here, we conclude that the sum of masses of reactants and products remain constant.
Example 2:
Take 10 g of CaCO3. Now, after the decomposition, CaCO3 decomposes to 6.2 g of CaO and 3.8 g of CO2. So, let’s represent this equivalence of mass as the conservation of mass:
CaCO3 -- decomposition → CaO + CO2
Calcium Carbonate Calcium Oxide Carbon dioxide
10 g 6.2 g 3.8 g
FAQs on Law of Conservation of Mass
1. What is the law of conservation of mass in simple terms?
The law of conservation of mass states that in an isolated system, mass cannot be created or destroyed by a chemical reaction or physical transformation. In simpler terms, the total mass of the substances you start with (reactants) in any change must be equal to the total mass of the substances you end up with (products).
2. Can you explain the law of conservation of mass with a simple example?
Certainly. A common example is the decomposition of calcium carbonate (CaCO₃). If you heat 100 grams of calcium carbonate, it will break down into 56 grams of calcium oxide (CaO) and 44 grams of carbon dioxide (CO₂).
Here, the total mass of the reactant is 100g. The total mass of the products is 56g + 44g = 100g. Since the mass of reactants equals the mass of products, this reaction perfectly demonstrates the law of conservation of mass.
3. How is the law of conservation of mass represented in a chemical reaction?
In chemistry, this law is the reason we must balance chemical equations. It is represented by the principle that the total mass on both sides of an equation must be equal. For any reaction, the formula is:
Total Mass of Reactants = Total Mass of Products
For example, in the reaction of methane (CH₄) burning in oxygen (O₂):
CH₄ + 2O₂ → CO₂ + 2H₂O
The mass of one molecule of methane plus two molecules of oxygen is exactly equal to the mass of one molecule of carbon dioxide and two molecules of water.
4. Why is the law of conservation of mass considered a fundamental principle in science?
This law is fundamental because it provides a foundational rule for tracking matter through any process. It is crucial for:
- Balancing Chemical Equations: It ensures that the number of atoms of each element is the same on both sides of an equation.
- Stoichiometry: It allows chemists to calculate the exact amounts of reactants needed and products expected in a chemical reaction.
- Industrial Processes: It is essential for designing efficient and waste-free manufacturing processes in various industries, from pharmaceuticals to food production.
5. Does the law of conservation of mass apply to physical changes, like ice melting, or only chemical reactions?
Yes, the law of conservation of mass applies to both physical and chemical changes. While chemical reactions rearrange atoms to form new substances, physical changes only alter the state or form of a substance. For example, if you melt a 10-gram ice cube (solid water) in a sealed container, you will get exactly 10 grams of liquid water. No mass is lost or gained in the process.
6. How does the law of conservation of mass relate to everyday activities like baking a cake?
Baking a cake is a great real-world example of the law of conservation of mass. The total mass of all your ingredients (flour, sugar, eggs, etc.) before mixing and baking is equal to the mass of the finished cake plus the mass of any water vapour and carbon dioxide gas that escaped during the baking process. Although the cake weighs less than the initial batter, the mass isn't destroyed; it has simply changed form and escaped as gas, perfectly upholding the law.
7. Are there any situations where the law of conservation of mass is not strictly followed?
For all standard chemical reactions and physical changes covered in the CBSE/NCERT syllabus, the law of conservation of mass holds true. However, in nuclear reactions (like those in the sun or nuclear power plants), a tiny amount of mass can be converted into a large amount of energy, as described by Einstein's famous equation, E=mc². In these specific, high-energy cases, mass and energy are considered inter-convertible, leading to the broader principle of the conservation of mass-energy.
