A chemist is studying the following equilibrium:
2Pb(NO3)2 (s) 2PbO (s) + 4NO2 (g) + O2 (g)
He starts out with 10 g of Pb(NO3)2 and, at equilibrium, has 2.02 g of PbO. The concentrations of NO2 and O2 at equilibrium are 0.18 M and 0.045 M, respectively. What is the value of the equilibrium constant?
For the following reaction:
2NH3 (g) N2 (g) + 3H2 (g)
The equilibrium concentrations are: [NH3] = 0.22 M, [N2] = 0.54 M, and [H2] = 0.66 M. What is the value of the equilibrium constant for this reaction?
Can someone please help me with these 2 chemistry questions?
2017-08-11 4:28 pm
回答 (1)
2017-08-11 4:52 pm
1.
2Pb(NO₃)₂(s) ⇌ 2PbO(s) + 4NO₂(g) + O₂(g) …… Kc
This is a heterogeneous equilibrium. Due to the fact that the effective density of a solid is constant, solid components are not present in the equilibrium constant.
Equilibrium constant, Kc = [NO₂]⁴ [O₂] = 0.18⁴ × 0.045 = 4.7 × 10⁻⁵
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2.
2NH₃(g) ⇌ N₂(g) + 3H₂(g)
Equilibrium constant, Kc = [N₂] [H₂]³ / [NH₃]² = 0.54 × 0.66³ / 0.22² = 3.2
2Pb(NO₃)₂(s) ⇌ 2PbO(s) + 4NO₂(g) + O₂(g) …… Kc
This is a heterogeneous equilibrium. Due to the fact that the effective density of a solid is constant, solid components are not present in the equilibrium constant.
Equilibrium constant, Kc = [NO₂]⁴ [O₂] = 0.18⁴ × 0.045 = 4.7 × 10⁻⁵
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2.
2NH₃(g) ⇌ N₂(g) + 3H₂(g)
Equilibrium constant, Kc = [N₂] [H₂]³ / [NH₃]² = 0.54 × 0.66³ / 0.22² = 3.2
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