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What are the Laws of Chemical Combinations?

The combination of different elements to form compounds is governed by certain basic rules. These rules are referred to as laws of chemical combination.

  • In chemistry, we study the change of matter from one form to the other. These changes sometimes occur as a result of the combination of two different types of matter
  • There are certain rules which are followed in the combination of different elements to form different compounds. 

There are five laws of chemical combinations:

  1. Law of Conservation of Mass
  2. Law of Definite Proportions
  3. Law of Multiple Proportions
  4. Gay Lussac's Law of Gaseous Volumes
  5. Avogadro's Law

1. Law of Conservation of Mass

“The mass in an isolated system can neither be created nor be destroyed but can be transformed from one form to another”. Let us look at an example first-

No. of Carbons, Hydrogens and Oxygens are the same on each side of the equation.No. of Carbons, Hydrogens and Oxygens are the same on each side of the equation.

  • In the above experiment, Mass of Reactants = Mass of Products which follows Law of Conservation of Mass.

Limitation of Law of Conservation of Mass

  • In nuclear reactions, some mass of reactant is converted into energy, so the mass of reactant is always less than that of product.
  • The other limitation of conservation of mass is according to Einstein’s theory, the relation between two quantities is given by E = mc2, which means that energy and mass are interconvertible. Therefore, for the law of conservation of mass to be valid mass and energy of the system must be conserved. 

Solved Examples of Law of Conservation of Mass

Example 1: A 15.9 gm sample of sodium carbonate is added to a solution of acetic acid weighing 20.0 gm. The two substances react, releasing carbon dioxide gas to the atmosphere. After the reaction, the contents of the reaction vessel weigh 29.3 gm. What is the mass of carbon dioxide given off during the reaction?

The total mass of reactants taken = 15.9 + 20.0 = 35.9 gm.

  • From the conservation of mass, the final mass of the contents of the vessel should also be 35.9 gm. 
  • But it is only 29.3 gm. The difference is due to the mass of released carbon dioxide gas. 
  • Hence, the mass of carbon dioxide gas released = 35.9 - 29.3 = 6.6 gm.

Example 2: 5.2 g of CaCO3 when heated produced 1.99 g of Carbon dioxide and the residue (CaO) left behind weighs 3.2 g. Show that these results illustrate the law of conservation of mass.

Weight of CaCO3 taken = 5.2 g

  • Total weight of the products (CaO + CO2 )= 3.20 + 1.99 = 5.19 g
  • Difference between the wt. of the reactant and the total wt. of the products
    = 5.20 – 5.19 =0.01 g.
  • This small difference may be due to experimental error.
  • Thus the law of conservation of mass holds good within experimental errors.

Question for Laws of Chemical Combinations
Try yourself:A quantity of 10 g of a hydrocarbon exactly requires 40 g oxygen for complete combustion. The products formed are CO2 and water. When CO2 gas formed is absorbed completely in lime water, the mass of solution increases by 27.5 g. What is the mass of water formed simultaneously in the combustion?
View Solution

2. Law of Definite Proportions

"All chemical compounds are found to have constant composition irrespective of their method of preparation or sources."

  • In the year 1794, the French chemist Joseph Proust formulated the law of constant proportions from his work on sulphides, metallic oxides, and sulfates.
  • In H2O, Hydrogen & oxygen combine in a 2:1 molar ratio, this ratio remains constant whether it is Tap water, river water, or seawater or produced by any chemical reaction.

The elements are always combined in the same proportions by mass.The elements are always combined in the same proportions by mass.

Limitations of Law of Definite Proportions 

  • The law does not hold true if the different isotopes of the same element are involved in making chemical compounds.
  • In the case of Isotopes, Combining Ratio is not fixed
    Example:
    12CO2      14CO2
    12:32         14:32

    3:8             7:16

Tip: Isotopes are the atoms possessing the same atomic number but different atomic masses.

Solved Examples of Law of Definite Proportions

Example 1: The following are results of the analysis of two samples of the same or two different compounds of phosphorus and chlorine. From these results, decide whether the two samples from the same or different compounds. Also state the law, which will be obeyed by the given samples.
Laws of Chemical Combinations | Chemistry Class 11 - NEET

  • The mass ratio of phosphorus and chlorine in compound A:
    mp : mcl = 1.156 : 3.971 = 0.2911 : 1.000
  • The mass ratio of phosphorus and chlorine in compound B:
    mp : mcl = 1.542 : 5.297 = 0.2911 : 1.000
    As the mass ratio is the same, both the compounds are the same and the samples obey the law of definite proportion.

Example 2: 6.488 g of lead combine directly with 1.002 g of oxygen to form lead peroxide PbO2. Lead peroxide is also produced by heating lead nitrate and it was found that the percentage of oxygen present in lead peroxide is 13.38 percent. Use these data to illustrate the law of constant composition.

Step 1: 

  • To calculate the percentage of oxygen in the first experiment.
  • Weight of peroxide formed = 6.488 + 1. 002 = 7.490 g
  • 7. 490 g of lead peroxide contain 1.002 g of oxygen

∴ 100 g of lead peroxide will contain oxygen:
Laws of Chemical Combinations | Chemistry Class 11 - NEET
i.e. oxygen present = 13.38%

Step 2: 

  • To compare the percentage of oxygen in both experiments. Percentage of oxygen in PbO2 in the first experiment = 13.38
  • Since the percentage composition of oxygen in both the samples of PbO2 is identical, the above data illustrate the constant composition law.

Question for Laws of Chemical Combinations
Try yourself:Two gaseous samples were analyzed. One contained 1.2 g of carbon and 3.2 g of oxygen. The other contained 27.3% carbon and 72.7% oxygen. The experimental data are in accordance with 
View Solution

3. Law of Multiple Proportions

"When one element combines with the other elements to form two or more different compounds, the mass of one element, which combines with a constant mass of the other, bears a simple ratio to one another."

Carbon can form two different compounds with oxygenCarbon can form two different compounds with oxygen

  • Carbon is found to form two oxides containing 42.9% & 27.3% of carbon, respectively, showing that these figures show the law of multiple proportions.
    Laws of Chemical Combinations | Chemistry Class 11 - NEET

In the first oxide:

  • 57.1 parts by mass of oxygen combine with 42.9 parts of carbon.
  • 1 part of oxygen will combine with 42.9/57.1 = 0.751 part of the carbon.

Similarly, in 2nd oxide:

  • 1 part of oxygen will combine with 27.3/72.7  = 0.376 part of the carbon.
  • The ratio of carbon that combines with the same mass of oxygen = 0.751: 0.376 = 2:1
  • This is a simple whole-number ratio, this means the above data shows the law of multiple proportions.

Limitations of Law of Multiple Proportions

  • The law of multiple proportions is not widely true or acceptable. 
  • The law is only applicable to small Reactions.
  • It means that this law is valid for basic chemical reactions.

  • The Law of multiple proportions is not valid for heavy and complex molecules

  • Because when heavy molecules are interlinked with each other then the total whole will not be as small.

Solved Examples of Law of Multiple Proportions

Example 1: Two oxide samples of lead were heated in the current of hydrogen and were reduced to metallic lead. The following data were obtained:
(i) Weight of yellow oxide taken = 3.45 gm; Loss in weight during reduction = 0.24 gm
(ii) Weight of brown oxide taken = 1.227 gm; Loss in weight during reduction = 0.16 gm.
Show that the data illustrate the law of multiple proportions. 

  • When the oxide of lead is reduced in the current of hydrogen, metallic lead is formed.
  • Definitely, the loss in weight is due to the removal of the oxygen present in the oxide, to combine with the hydrogen.
  • Therefore, the composition of the yellow oxide is:
    Oxygen = 0.24 gm and lead = 3.45 - 0.24 = 3.21 gm.
  • The mass ratio of lead and oxygen:
    Laws of Chemical Combinations | Chemistry Class 11 - NEET
  • The composition of the brown oxide is : oxygen = 0.16 gm and lead = 1.227 - 0.16 = 1.067 gm.
  • The mass ratio of lead and oxygen:
    Laws of Chemical Combinations | Chemistry Class 11 - NEET
  • Now, r1 : r2 = 13.375 : 6.669 = 2:1 (simple ratio) and hence the data illustrates the law of multiple proportion. 

Example 2: Carbon is found to form two oxides, which contain 42.9% and 27.3% of carbon respectively. Show that these figures illustrate the law of multiple proportions.

Step 1: 

  • To calculate the percentage composition of carbon and oxygen in each of the two oxides:
  • First oxide:  Carbon 42.9%   27.3% (Given)
  • Second oxide: Carbon Oxygen 57.1% 72.7% (by difference)

Step 2: 

To calculate the weights of carbon which combine with a fixed weight i.e., one part by weight of oxygen in each of the two oxides.

  • In the first oxide, 57.1 parts by weight of oxygen combine with carbon = 42.9 parts.
    ∴ 1 part by weight of oxygen will combine with carbon 42.9/57.1 = 0.751
  • In the second oxide, 72.7 parts by weight of oxygen combine with carbon = 27.3 parts.
    ∴ 1 part by weight of oxygen will combine with carbon  27.3/72.7 = 0.376

Step 3: 

  • To compare the weights of carbon, combined with the same weight of oxygen in both the oxides. 
  • The ratio of the weights of carbon that combine with the same weight of oxygen (1 part) is 0.751: 0.376 or 2:1

Since this is a simple whole-number ratio, so the above data illustrate the law of multiple proportions.

Question for Laws of Chemical Combinations
Try yourself:Two elements A and B combine to form compound X and Y. For the fixed mass of A, masses of B combined for the compounds X and Y are in 3:7 ratio. If in compound X, 4 g of A combines with 12 g B, then in compound Y, 8 g of A will combine with ...... g of B.
View Solution

4. Gay Lussac's Law of Gaseous Volumes 

  • The law was proposed by Gay Lussac in 1808.
  • When gases combine or are produced in a chemical reaction, they do so in a simple ratio by volume.
  • This ratio holds true when all gases involved are at the same temperature and pressure.
  •  For instance, when hydrogen and oxygen react to form water vapor, 100 mL of hydrogen combines with 50 mL of oxygen to produce 100 mL of water vapor.
  • The volumes of hydrogen and oxygen in this example (100 mL and 50 mL) bear a simple ratio of 2:1.
  • Gay Lussac's discovery is an extension of the law of definite proportions, which was initially stated for mass.
  • Avogadro further explained Gay Lussac's law in 1811, emphasizing the relationship between volume and the number of particles.
  • Gay Lussac's law describes how gases combine in simple volume ratios under specific conditions, contributing to our understanding of chemical reactions. Avogadro's work later provided a more comprehensive explanation of this law.

Example of Gay Lussac`s LawExample of Gay Lussac's Law

Limitations of Gay-Lussac's Law

  • The law is only applicable to ideal gases.
  • Gay-Lussac's law holds good for real gases at high temperatures and/or low pressure.
  • The ratio of the pressure to temperature deviated at high pressures. The ratio decreases with increasing the pressure.

Solved Examples of Gay-Lussac's Law

Example 1: 2.5 ml of a gaseous hydrocarbon exactly requires 12.5 ml oxygen for complete combustion and produces 7.5 ml carbon dioxide and 10.0ml water vapour. All the volumes are measured at the same pressure and temperature. Show that the data illustrates Gay Lussac's law of volume combination. 

V(hydrocarbon) : Voxygen : V(carbon dioxide) : V(water vapour)
= 2.5 : 12.5 : 7.5 : 10.0
= 1 : 5 : 3 : 4 (simple ratio)

Hence, the data is according to the law of volume combination.

Example 2: How much volume of oxygen will be required for the complete combustion of 40 ml of acetylene (C2H2) and how much volume of carbon dioxide will be formed? All volumes are measured at NTP.

Laws of Chemical Combinations | Chemistry Class 11 - NEET
So, for complete combustion of 40 ml of acetylene, 100 ml of oxygen is required and 80 ml of CO2 is formed.

5. Avogadro's Law

"Equal volumes of gases at the same temperature and pressure should contain an equal number of molecules."

  • This implies that 2 litres of hydrogen will have the same number of molecules as 2 litres of oxygen given that both gases are at the same temperature and pressure.
  • Avogadro made a distinction between atoms and molecules which is quite understandable in the present times. 
  • If we consider the reaction of hydrogen and oxygen to produce water, we see that two volumes of hydrogen combine with one volume of oxygen to give two volumes of water without leaving any unreacted oxygen.

Avogadro`s LawAvogadro's Law

Limitations of Avogadro's Law

  • The law works perfectly only for ideal gases.
  • The law is approximate for real gases at low pressure and/or high temperature.  

Solved Example of Avogadro's Law

Examples 1: A tyre that consists of 10 moles air and occupies 40L volume loses half of the volume because of a puncture. What is the amount of air left in the deflated tyre at STP?

Initial amount of air  n1 is 10 mol

Initial volume of tyre V1 is 40 L

Final volume of tyre V2 is 20 L

According to Avogadro’s law, 

the amount of air left in the deflated tyre,

n2 = Laws of Chemical Combinations | Chemistry Class 11 - NEET  = 5 moles

Hence, the deflated tyre contains 5 moles air

Question for Laws of Chemical Combinations
Try yourself:The percentage of copper and oxygen in samples of CuO obtained by different methods was found to be the same. This illustrates the law of:
View Solution

Laws of Chemical Combinations: Solved Examples

Q1. What mass of silver nitrate will react with 5.85 g of sodium chloride to produce 14.35 g of silver chloride and 8.5 g of sodium nitrate, if the law of conservation of mass is true?

According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.

For the chemical reaction: AgNO+ NaCI → NaNO+ AgCI

mreactants = mproducts

mAgNO3 + mNaCl = mNaNO3 + mAgCl
x + 5.85 = 8.5 + 14.35
x = 17.0 g

Q.2. Elements X and Y form two different compounds. In the first, 0.324 g of X is combined with 0.471 g of Y. In the second, 0.117 g of X is combined with 0.509 g of Y. Show that these data illustrate the law of multiple proportions.

Ans: According to the law of multiple proportions, "If two elements form more than one compound between them, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers".

  • In the first compound, 0.324 g of X is combined with 0.471 g of Y.
    Hence, 1 g of X is combined with  0.471/0.324  = 1.45 g of Y.
  • In the second compound, 0.117 g of X is combined with 0.509 g of Y.
    Hence, 1 g of X is combined with 0.1170.509 = 4.35 g of Y.
  • The ratio of 4.35/1.35 = 3 is a small whole number.
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FAQs on Laws of Chemical Combinations - Chemistry Class 11 - NEET

1. What is the Law of Conservation of Mass in chemical combinations?
Ans. The Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction, only rearranged.
2. How does the Law of Definite Proportions apply in chemical combinations?
Ans. The Law of Definite Proportions states that a chemical compound always contains the same elements in the same proportion by mass.
3. What is Gay Lussac's Law of Gaseous Volumes in chemical combinations?
Ans. Gay Lussac's Law of Gaseous Volumes states that when gases react, they do so in volumes that are in simple whole number ratios.
4. How does Avogadro's Law relate to chemical combinations?
Ans. Avogadro's Law states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
5. Can you explain the Law of Multiple Proportions in chemical combinations?
Ans. The Law of Multiple Proportions states that when two elements form more than one compound, the ratios of the masses of one element that combine with a fixed mass of the other element can be expressed in small whole numbers.
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