# one mole of a gas occupies a volume of 22.4 l. this is derived from

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## One gram mole of a gas at NTP occupies \\[22.4\\] litres as volume. This fact was derived from:A. Dalton’s theoryB. Avogadro’s hypothesisC. Berzelius hypothesisD. law of gaseous volumes

One gram mole of a gas at NTP occupies \\[22.4\\] litres as volume. This fact was derived from:A. Dalton’s theoryB. Avogadro’s hypothesisC. Berzelius hypothesisD. law of gaseous volumes. Ans: Hint: One gram mole of a gas is equal to the molecular wei...

One gram mole of a gas at NTP occupies22.4 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

Last updated date: 17th Mar 2023

• Total views: 228k • Views today: 2.08k Answer Verified 228k+ views

**Hint:**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× 10 23 6.023×1023

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 V and moles of gas n n

are directly proportional.

From ideal gas equation,

PV=nRT PV=nRT ( V V

is directly proportional to

n n ) Where P P = pressure = 1atm 1atm at NTP T T = temperature = 273 K 273 K at NTP R R = gas constant = 0.0821 atm L K −1 mo l −1

0.0821 atm LK−1mol−1

n n = mole of gas = 1 1

From the above equation,

V= nRT P V=nRTP V= 1×0.0821×273 1 V=1×0.0821×2731 V=22.4L 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.

## One gram mole of a gas at NTP occupies 22.4 L. This fact is derived from

b) one gram mole of a gas at NTP occupies 22.4 L. This fact is derived from Avogadro's hypothesis.

One gram mole of a gas at NTP occupies 22.4 L. This fact is derived from

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Text Solution A

law of gaseous volumes

B

Avogadro's hypothesis

C

Dalton's atomic theory

D

Berzelius hypothesis

Solution

b) one gram mole of a gas at NTP occupies 22.4 L. This fact is derived from Avogadro's hypothesis.

Answer

Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams.

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## One gram mole of a gas at STP occupies 22.4 L volume. This fact is derived fromA. Avogadro's hypothesisB. Berzelius hypothesisC. None of the aboveD. Daltion's theory

One gram mole of a gas at STP occupies 22.4 L volume. This fact is derived fromA. Avogadro's hypothesisB. Berzelius hypothesisC. None of the aboveD. Daltion's theory

Byju's Answer Standard IX Chemistry One gram mole... Question

One gram mole of a gas at STP occupies 22.4L volume. This fact is derived from___.

A Daltion’s theory B

Avogadro’s hypothesis

C

Berzelius hypothesis

D None of the above Open in App Solution

The correct option is **A**

Avogadro’s hypothesis

1 mole of all gases at constant temperature and pressure occupy the same volume

One mole of a gas at STP occupies 22.4L.

One mole of hydrogen gas is 2.016g

2.016g→ 22.4L 1g → **y** Calculate **y**.

**y**= (1 x 22.4)/ 2.016

**y**= 11.11L

Suggest Corrections 3

SIMILAR QUESTIONS

**Q.**

One gram mole of a gas at STP occupies 22.4L volume. This fact was derived from –

**Q.**One gram molecule of any gas at

N T P occupies 22.4 L

. This fact was derived from:

**Q.**One gram mole of a gas at NTP occupies

22.4

litres as volume. This fact was derived from:

**Q.**"One gram moecule of gas at N.T.P occupies

22.4

litres." This fact was derived from?

**Q.**Assertion :One mole of oxygen gas occupies

22.4 l

volume at STP. Reason: Volume of a gas depends on temperature and pressure and also nature of gas.

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Standard IX Chemistry

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