Question

One gram mole of a gas at NTP occupies $22.4$ litres as volume. This fact was derived from:
A. Dalton’s theory
B. Avogadro’s hypothesis
C. Berzelius hypothesis
D. law of gaseous volumes

Answer 1

One gram mole of a gas is equal to the molecular weight of gas in grams. NTP is considered as the normal temperature and pressure. A mole is equivalent to $6.023 \times {10^{23}}$ numbers of particles in a substance also called Avogadro's number.

Complete step by step answer:
For ideal gases the volume of gas and the amount of substance are related by a mathematical equation given by Avogadro. Avogadro’s law states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. At constant temperature and pressure the volume $V$ and moles of gas $n$ are directly proportional.
From ideal gas equation, $PV = nRT$ ($V$ is directly proportional to $n$)
Where $P$ = pressure = $1atm$ at NTP
$T$ = temperature = $273{\text{ }}K$ at NTP
$R$ = gas constant = $0.0821{\text{ }}atm{\text{ }}L{K^{ - 1}}mo{l^{ - 1}}$
$n$ = mole of gas =$1$
From the above equation, $V = \dfrac{{nRT}}{P}$
$V = \dfrac{{1 \times 0.0821 \times 273}}{1}$
$V = 22.4L$.
Hence the correct answer is B.
Dalton's law (also known as Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
Berzelius hypothesis states that equal volumes of all gases contain equal numbers of atoms under the same conditions of temperature and pressure. This law becomes opposite to Dalton's law when applied to the law of combining volumes because this hypothesis predicts that atoms are divisible.
Law of gaseous volumes states that the ratio between the volumes of the reactant gases and the gaseous products can be expressed in simple whole numbers.

So, the correct answer is Option B.

Note: All the gas laws are applicable to ideal gases. They are not fully true for real gases. The increase in the number of particles in a container increases the outward pressure on the container walls at the same temperature.