Samples of the gases $O_{2}, N_{2}, C O_{2}$ and CO under the same condition of temperature and pressure contain the same number of molecules x. The molecules of oxygen occupy V litres and have a mass of 8 g under the same what is the volume occupied by
(a) x molecules of $N_{2}$
(b) 3x molecules of CO,
(c) What is the mass of $C O_{2}$ in grams?
(d) In answering the above questions, which law have used?

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Solution

Avogadro's law states that, "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.
(a) Thus if x molecules of oxygen occupies V litres then x molecules of nitrogen will also occupy V litres of volume.
(b) X molecule of CO occupy V litre, thus 3x will occupy 3V litres.
(c) moles of $C O_{2}$ = moles of oxygen = $\frac{8}{32}$ = $\frac{1}{4}$
Mass of $C O_{2}$ = $\frac{1}{4} \times 44$ = 11 g
(d) Avogadro's law

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Similar questions

Samples of the gases O₂, N₂, CO₂ and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen [O₂], occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure:
(a) What is the volume occupied by:
(i) X molecules of N₂?
(ii) 3X molecules of CO? [C = 12, N = 14, O = 16]
(b) What is the mass of CO₂ in g?
(c) In answering the above questions, which law have you used?

Samples of gases O₂, N₂, CO, and CO under the same conditions of temperature and pressure contain the same number of molecules represented by X. The molecules of oxygen (O₂) occupy V litres and have a mass of 8 g. Under the same conditions of temperature and pressure:

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one litre flasks are separately filled with the gases,

O_{2}, F_{2}, C H_{4}

and

C O_{2}

under the same condition of temperature and pressure. The ratio of number of molecules in these gases is:

(a) (i) What volume of oxygen is required to burn completely $90 d m^{3}$ of butane under similar conditions of temperature and pressure?

$2 C_{4} H_{10} + 13 O_{2} \to 8 C O_{2} + 10 H_{2} O$

(ii) the vapour density of a gas is 8. What would be the volume occupied by 24.0 g of the gas at STP?
(iii) A vessel contains X number of molecules of hydrogen gas at a certain temperature and pressure. How many molecules of nitrogen gas would be present in the same vessel under the same conditions of temperature and pressure?

(b) $O_{2}$ is evolved by heating $K C l O_{3}$ using $M n O_{2}$ as a catalyst.

$2 K C l O_{3} M n O_{2} - --- \to 2 K C l + 3 O_{2}$

(i) Calculate the mass of $K C l O_{3}$ required to produce 6.72 litres of $O_{2}$ at STP.
[atomic masses of $K = 39, C l = 35.5, O = 16]$
(ii) Calculate the number of moles of oxygen present in the above volume and also the number of molecules.
(iii) Calculate the volume occupied by 0.01 mole of $C o_{2}$ at STP.

Q. Two gases A and B are taken in same volume containers under similar conditions of temperature and pressure. In container A, there are '2N' molecules of gas A. The number molecules does container B have :

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