A gas occupies 2.0 L at 1.0 atm. If pressure is increased to 4.0 atm at constant temperature, the volume will be:
A. 1.0 L
B. 0.5 L
C. 2.0 L
D. 8.0 L
Answer: Option B
Solution (By JKSSB Mock Tests)
Boyle's law: P₁V₁ = P₂V₂. Given P₁=1.0 atm, V₁=2.0 L, P₂=4.0 atm. V₂ = (1.0 × 2.0) / 4.0 = 0.5 L. Volume decreases as pressure increases, because gas is compressible. The product PV is constant for a fixed mass of gas at constant T. Scuba divers experience this; as they dive deeper, pressure increases, reducing air volume in lungs.
Explanation:
Ammonium chloride (NH₄Cl) consists of NH₄⁺ and Cl⁻ ions. Ionic bond between NH₄⁺ and Cl⁻. Within NH₄⁺, N-H are covalent bonds, with one coordinate bond formed by donation of N's lone pair to H⁺. So all three bond types are present. NaCl purely ionic. CO₂ purely covalent. CH₄ purely covalent.
Explanation:
Fermentation of sugars (glucose, fructose) by yeast enzymes produces ethanol and carbon dioxide: C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂. Starch is first hydrolysed to glucose. Proteins and fats are not directly fermented to ethanol.
Explanation:
The Haber process synthesizes ammonia from nitrogen and hydrogen (N₂ + 3H₂ ⇌ 2NH₃). Finely divided iron acts as the catalyst, often with molybdenum as a promoter, to increase the rate of reaction at high pressure and moderate temperature. V₂O₅ is used in the Contact process.
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