A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure.
(a) What mass of carbon dioxide can it hold under similar conditions of temperature and pressure?
(b) If the number of molecules of hydrogen in the cylinder is X, calculate the number of carbon dioxide molecules in the cylinder. State the law that helped you to arrive at the above result

Question

A gas cylinder can hold 1 kg of hydrogen at room temperature and pressure.
(a) What mass of carbon dioxide can it hold under similar conditions of temperature and pressure?
(b) If the number of molecules of hydrogen in the cylinder is X, calculate the number of carbon dioxide molecules in the cylinder. State the law that helped you to arrive at the above result

KnowledgeBoat · Accepted Answer

(a) Given, cylinder can hold = 1 kg of hydrogen Molar mass of hydrogen = 2[1] = 2g Number of moles of hydrogen present in cylinder = = 500 According to avogadro's law : cylinder will hold 500 moles of carbon dioxide gas Molar mass of CO₂ = C + 2(O) = 12 + 2(16) = 44 g 1 mole of carbon dioxide = 44 g ∴ 500 moles of carbon dioxide = 44 x 500 = 22,000 g = 22 kg. Hence, Weight of carbon dioxide in cylinder = 22 kg (b) According to Avogadro's law Equal volumes of all gases under similar conditions of temperature and pressure contain equal number of molecules. ∴ molecules in the cylinder of carbon dioxide = X Avogadro's law helped to arrive at this result.

Chemistry

Mole Concept

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(a) Calculate the mass of substance 'A' which in gaseous form occupies 10 litres at 27°C and 700 mm pressure. The molecular mass of 'A' is 60.
(b) A gas occupied 360 cm³ at 87°C and 380 mm Hg pressure. If the mass of gas is 0.546 g, find it's relative molecular mass.

A compound A consists of 4.8% carbon and 95.2% bromine by mass. Its vapour density is 252. Find its :
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Chemistry

Mole Concept

Related Questions

(a) Calculate the mass of substance 'A' which in gaseous form occupies 10 litres at 27°C and 700 mm pressure. The molecular mass of 'A' is 60.(b) A gas occupied 360 cm3 at 87°C and 380 mm Hg pressure. If the mass of gas is 0.546 g, find it's relative molecular mass.

A compound A consists of 4.8% carbon and 95.2% bromine by mass. Its vapour density is 252. Find its :(i) empirical formula(ii) molecular formula

(a) Calculate the mass of substance 'A' which in gaseous form occupies 10 litres at 27°C and 700 mm pressure. The molecular mass of 'A' is 60.
(b) A gas occupied 360 cm³ at 87°C and 380 mm Hg pressure. If the mass of gas is 0.546 g, find it's relative molecular mass.

A compound A consists of 4.8% carbon and 95.2% bromine by mass. Its vapour density is 252. Find its :
(i) empirical formula
(ii) molecular formula