SC15 · Overview Dynamic equilibria and calculations involving volumes of gases mind map

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SC15 · Overview Dynamic equilibria and calculations involving volumes of gases mind map

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Gas ratios · Higher

Matching conditions: Same T / p: gas volume ratios follow equation coefficients
Amount: n = V ÷ molar volume; 24 dm³/mol = 24,000 cm³/mol at stated RTP
Mass to gas: n = m/Mᵣ → mole ratio → gas moles × molar volume
Haber ratio: N₂ : H₂ : NH₃ = 1 : 3 : 2 for complete theoretical conversion
Limits: Gas volumes only; same T / p; limiting reactant / equilibrium matter

Haber process

Feed / reaction: N₂ from air / H₂ often natural gas; N₂ + 3H₂ ⇌ 2NH₃; exothermic
Temperature · Higher: ≈450 °C compromise; lower T favours yield but slows rate
Pressure · Higher: ≈200 atm; fewer product gas molecules favoured; equipment costs
Catalyst · Higher: Iron speeds both rates; no change to equilibrium yield
Recovery · Higher: Cool / condense NH₃; recycle unreacted N₂ / H₂

Equilibria · Higher

Rate / position: More collisions speed approach; position effects judged separately
Economics: Rate, yield, energy, supply, safety / equipment; maximum yield ≠ best cost
Rules: Higher p → fewer gas molecules; hotter → endothermic direction

Fertilisers

NPK: N / P / K replace harvested nutrients; still need light / water / CO₂
Nitrate: NH₃ + HNO₃ → NH₄NO₃
Sulfate: 2NH₃ + H₂SO₄ → (NH₄)₂SO₄; ratio 2:1
Laboratory: Titrate volumes → repeat without indicator → concentrate / crystallise
Industry: Large continuous systems / heat recovery / automatic control
Impacts: Energy / cost; efficient use limits nutrient run-off / eutrophication

Connections

Gas ratios · Higher → Haber process: The balanced Haber equation determines theoretical gas ratios.
Haber process → Fertilisers: Industrial ammonia supplies nitrogen for ammonium fertilisers.