Water decomposes to O₂ and H₂ under suitable conditions as represented by the equation below: 2H₂O 2H₂ + O₂ (a) If 2500 cm³ of H₂ is produced, what volume of O₂ is liberated at the same time and under the same conditions of temperature and pressure? (b) The 2500 cm³ of H₂ is subjected to times increase in pressure (temp. remaining constant). What volume will H₂ now occupy? (c) Taking the value of H₂ calculated in 5(b), what changes must be made in Kelvin (absolute) temperature to return the volume to 2500 cm³ pressure remaining constant.

Question

KnowledgeBoat · Accepted Answer

2 Vol. of water gives 2 Vol. of H₂ and 1 Vol. of O₂ ∴ If 2500 cm³ of H₂ is produced, volume of O₂ produced = = 1250 cm³ (b) V₁ = 2500 cm³ P₁ = 1 atm = 760 mm T₁ = T T₂ = T P₂ = [760 x 2 ] + [760] = 760 [ + 1] = 760 x = 2660 mm V₂ = ? Using formula: = = V₂ = = (c) V₁ = = 714.29 cm³ P₁ = P₂ = P T₁ = T V₂ = 2500 cm³ T₂ = ? Using formula: = = T₂ = x T T₂ = 3.5 x T Hence, T₂ = 3.5 times T or temperature should be increased by 3.5 times

Chemistry

Mole Concept

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