Where do I start?
2016-05-09 8:45 pm
The following reaction was performed in a sealed vessel at 735 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.60M and [I2]=2.65M. The equilibrium concentration of I2 is 0.0400 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
回答 (1)
2016-05-09 8:57 pm
H₂(g) + I₂(g) ⇌ 2HI(g) .... Kc
Initial concentrations :
[H₂]ₒ = 3.60 mol/L
[I₂]ₒ = 2.65 mol/L
Change in concentration of I₂ = 0.0400 - 2.65 = -2.61 mol/L
At equilibrium :
[H₂] = 3.60 - 2.61 = 0.99 mol/L
[I₂] = 0.0400 mol/L
[HI] = 2.61 × 2 = 5.22 mol/L
Kc = [HI]² / ([H₂] [I₂]) = (5.22)²/ (0.99 × 0.0400) = 688
Initial concentrations :
[H₂]ₒ = 3.60 mol/L
[I₂]ₒ = 2.65 mol/L
Change in concentration of I₂ = 0.0400 - 2.65 = -2.61 mol/L
At equilibrium :
[H₂] = 3.60 - 2.61 = 0.99 mol/L
[I₂] = 0.0400 mol/L
[HI] = 2.61 × 2 = 5.22 mol/L
Kc = [HI]² / ([H₂] [I₂]) = (5.22)²/ (0.99 × 0.0400) = 688
收錄日期: 2021-04-18 14:51:05
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20160509124552AAroeci