An unknown gas shows a density of 3 g per litre at 273°C and 1140 mm Hg pressure. What is the gram molecular mass of this gas?
Mole Concept
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An unknown gas shows a density of 3 g per litre at 273°C and 1140 mm Hg pressure. What is the gram molecular mass of this gas?

KnowledgeBoat · Accepted Answer

Given: P = 1140 mm Hg Density = D = 3 g per L T = 273 °C = 273 + 273 = 546 K gram molecular mass = ? At S.T.P., the volume of one mole of any gas is 22.4 L Volume of unknown gas at S.T.P. = ? By Charle’s law. V₁ = 1 L T₁ = 546 K T₂ = 273 K V₂ = ? = Hence, V₂ = x 273 = 0.5 L Volume at standard pressure = ? Apply Boyle’s law. P₁ = 1140 mm Hg V₁ = 0.5 L P₂ = 760 mm Hg V₂ = ? P₁ × V₁ = P₂ × V₂ V₂ = = 0.75 L Now, 22.4 L = 1 mole of any gas at S.T.P., then 0.75 L = = 0.0335 moles The original mass is 3 g Molecular mass = = = 89.55 ≈ 89.6 g per mole Hence, the gram molecular mass of the unknown gas is 89.6g

Chemistry

An unknown gas shows a density of 3 g per litre at 273°C and 1140 mm Hg pressure. What is the gram molecular mass of this gas?

Mole Concept

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An unknown gas shows a density of 3 g per litre at 273°C and 1140 mm Hg pressure. What is the gram molecular mass of this gas?

Mole Concept

Related Questions

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Correct the following:
(a) Equal volumes of any gas, under similar conditions, contain an equal number of atoms.
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(c) The unit of atomic weight is grams.

Give the empirical formula of:
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