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ahmedeldyame
25.06.2021 •
Chemistry
Nitrogen gas and chlorine gas will react to form nitrogen monochloride gas. 5 moles of nitrogen and 10 moles of chlorine are mixed in a previously evacuated 2 L flask at 500 K. After equilibrium has been established, there are 3 moles of NCl (g) present. What is the equilibrium constant (Kc) for this reaction at 500 K
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Ответ:
0.30
Explanation:
Step 1: Calculate the known initial and equilibrium molar concentrations
[N₂]i = 5 mol/2 L = 2.5 M
[Cl₂]i = 10 mol/2 L = 5 M
[NCl]e = 3 mol/2 L = 1.5 M
Step 2: Make an ICE chart
N₂(g) + Cl₂(g) ⇄ 2 NCl(g)
I 2.5 5 0
C -x -x +2x
E 2.5-x 5-x 2x
Step 3: Find the value of x
We know that [NCl]e = 2x = 1.5 ⇒ x = 0.75 M
Step 4: Calculate the concentrations at equilibrium
[N₂]e = 2.5-x = 2.5-0.75 = 1.75 M
[Cl₂]e = 5-x = 5-0.75 = 4.25 M
[NCl]e = 1.5 M
Step 5: Calculate the equilibrium constant (Kc)
Kc = [NCl]² / [N₂] × [Cl₂]
Kc = 1.5² / 1.75 × 4.25 = 0.30
Ответ: