For the Haber process: N₂ + 3H₂ ⇌ 2NH₃, Δ H = -92 kJ/mol State the effect on equilibrium of: (a) increasing — JEE Chemistry
For the Haber process: $N_2 + 3H_2 \rightleftharpoons 2NH_3$, $\Delta H = -92$ kJ/mol
State the effect on equilibrium of: (a) increasing pressure, (b) increasing temperature, (c) adding a catalyst.
1 Answer
CCamilleDubois28
✓ Accepted
· 1mo ago
▲ 3
(a) Increasing pressure: Shifts equilibrium to the right (fewer moles of gas: 4 → 2). ✓ More $NH_3$ produced.
(b) Increasing temperature: Since reaction is exothermic, increasing temperature shifts equilibrium to the left. ✗ Less $NH_3$.
(c) Adding catalyst: Does not shift equilibrium position. Increases rate of both forward and backward reactions equally. Equilibrium is reached faster.
$$(a) Right, (b) Left, (c) No shift — faster equilibrium$$
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Discussion (3)
K
Why do we take the positive value only in the last step?
AR
Saved me before my mock test. Much clearer than my coaching notes.
VA
Great discussion here. If you want more practice on this concept, check the related questions in this category.