Calculate the equilibrium concentration of each compound if 2.30 moles of CO and 3.40 moles of Br2 are placed in a 4.50 liter container?

[匿名]

2020-05-20 11:16 pm

Calculate the equilibrium concentration of each compound if 2.30 moles of CO and 3.40 moles of Br2 are placed in a 4.50 liter container at 73°C.Kc = 0.180 for the reaction at this temperature.

COBr2(g) equilibrium reaction arrow CO(g) + Br2(g)

回答 (1)

用戶26240

2020-05-20 11:35 pm

✔ 最佳答案

Initial concentration of CO, [CO]ₒ = (2.30 mol) / (4.50 L) = 0.511 mol/L
Initial concentration of Br₂, [Br₂]ₒ = (3.40 mol) / (4.50 L) = 0.756 mol/L

_                COBr₂(g) ⇌ CO(g)   + Br₂(g) Kc = 0.180
Initial (mol/L):       0      0.511          0.756
Change (mol/L): +y              -y           -y
Eqm (mol/L):        y     (0.511 - y)   (0.756 - y)

At equilibrium:
Kc = [CO] [Br₂] / [COBr₂]
0.180 = (0.511 - y) (0.756 - y) / y
0.180y = 0.386316 - 1.267y + y²
y² - 1.447 + 0.386316 = 0
y = [1.447 - √(1.447² - 4*0.386316)]/2
y = 0.353

[COBr₂] = 0.353 mol/L
[CO] = (0.511 - 0.353) mol/L = 0.158 mol/L
[Br₂] = (0.756 - 0.353) mol/L = 0.403 mol/L

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