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Gay-Lussac's Law

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Estimated time: 8 minutes
  • Definition: Limiting Reagent or Limiting Reactant
  • Law: Gay-Lussac's Law of Combining Volumes
CISCE: Class 10

Definition: Limiting Reagent or Limiting Reactant

The reactant which is completely used up in a reaction is known as Limiting reagent or Limiting reactant.

CBSE: Class 12
CISCE: Class 10

Law: Gay-Lussac's Law of Combining Volumes

"When gases combine or are produced in a chemical reaction, they do so in a simple ratio by volume, provided all gases are at the same temperature and pressure."

  • Proposed by Gay-Lussac in 1808.
  • e.g. 100 mL H₂ + 50 mL O₂ → 100 mL H₂O vapour (ratio = 2 : 1 : 2).
  • The volume ratio of gaseous reactants to products agrees with their molar ratio.
  • Volume of a gas is directly proportional to the number of moles (not inversely).
CBSE: Class 12
Maharashtra State Board: Class 11, 12

Law: Gay-Lussac’s Pressure–Temperature Law

Statement: The volume remaining constant, the pressure of a given mass of gas increases or decreases by 1/273.15 of its pressure at 0°C for each 1°C rise or fall in temperature.

P ∝ T or \[\frac {P}{T}\] = constant or \[\frac {P_1}{T_1}\] = \[\frac {P_2}{T_2}\]
Pt = P0(1 + \[\frac {βt}{273.15}\])

where β = pressure expansion coefficient = 1/273 per °C.

Related QuestionsVIEW ALL [26]

200 cm3 of CO2 is collected at STP when a mixture of acetylene and oxygen is ignited. Calculate the volume of acetylene and oxygen at STP. in original mixture.

\[\ce{2C2H2_{(g)} + 5O2_{(g)} → 4CO2_{(g)} + 2H2O_{(g)}}\]

When gases react their volumes bear a simple ratio to each other, under the same conditions of temperature and pressure. Who proposed this gas law?

A mixture of hydrogen and chlorine occupying 36 cm3 was exploded. On shaking it with water, 4 cm3 of hydrogen was left behind. Find the composition of the mixture.

How does Avogadro's law explain Gay - lussac's law of combining volumes?

24 cc Marsh gas (CH4) was mixed with 106 cc oxygen and then exploded. On cooling the volume of the mixture became 82 cc, of which, 58 cc was unchanged oxygen. Which law does this experiment support? Explain with calculations.

Water can split into hydrogen and oxygen under suitable conditions. The equations representing the change is:  2H2O(I) → 2H2 (g) + O2(g)
If a given experiment results in 2500cm3 of hydrogen being produced, what volume of oxygen is liberated at the same time under the same conditions of temperature and pressure?

112 cm3 of H2S(g) is mixed with 120 cm3 of Cl2(g) at STP to produce HCl(g) and sulphur(s). Write a balanced equation for this reaction and calculate

  1. the volume of gaseous product formed.
  2. composition of the resulting mixture.

What volume of air (containing 20% O2 by volume) will be required to burn completely 10 cm3 of methane and acetylene?

\[\ce{CH4 + 2O2 → CO2 + 2H2O}\]

\[\ce{2C2H2 + 5O2 -> 4CO2 + 2H2O}\]

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