What happens to the position of equilibrium when the volume of the reaction container is halved for the system: 2SO₂(g) + O₂(g) ⇌ 2SO₃(g)?
Answer and explanation
Correct answer: D. It shifts forward toward the products
- Step 1: Halving the volume doubles total pressure. Apply Le Chatelier's principle.
- Step 2: Reactant gas moles = 2 + 1 = 3; product gas moles = 2. The system relieves increased pressure by shifting toward the side with fewer gas molecules (forward, producing more SO₃).
Answer
It shifts forward toward the products.
Why not the others: Shifting backward increases pressure; remaining unaffected ignores the mole imbalance; the reaction reaches a new equilibrium rather than stopping.
Practise more Chemical Reactions, Equilibrium and Thermochemistry.
Free questions with an explanation for every one, and full timed EmSAT Achieve (UAE) mock tests.
More Chemical Reactions, Equilibrium and Thermochemistry questions
- What is the pH of a 0.0050 M aqueous solution of barium hydroxide, Ba(OH)₂, assuming complete dissociation?
- For the exothermic equilibrium N₂(g) + 3H₂(g) ⇌ 2NH₃(g) (ΔH = -92 kJ/mol), which change will increase the equilibrium yield of ammonia (NH₃)…
- Calculate the standard enthalpy of reaction for: CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l), given ΔH°f [CH₄(g)] = -75 kJ/mol, ΔH°f [CO₂(g)] = -394…
- The reaction 2NO(g) + O₂(g) → 2NO₂(g) has the experimental rate law Rate = k[NO]²[O₂]. If the concentration of NO is doubled while [O₂] is h…
- What is the solubility product constant (K_sp) of lead(II) chloride, PbCl₂, if its molar solubility in pure water at 25°C is 1.6 × 10⁻² M?
- Which pair of chemical species forms an effective buffer solution when mixed in equimolar amounts?