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Maru [420]
3 years ago
7

For the following reaction, find the value of Q and predict the direction of change, given that a 1L flask initially contains 2

moles S8, 2 moles SF6, and 2 moles F2.
1/8 S8 (s) + 3 F2 (g) ⇄ SF6 (g) Kc = 0.425

(A) Q = K, system is at equilibrium
(B) Q < K, reaction will make more reactants
(C) Q < K, reaction will make more products
(D) Q > K, reaction will make more reactants
(E) Q > K, reaction will make more products
Chemistry
1 answer:
Tresset [83]3 years ago
5 0

Answer:

C) Q < K, reaction will make more products

Explanation:

  • 1/8 S8(s)  + 3 F2(g)  ↔  SF6(g)

∴ Kc = 0.425 = [ SF6 ] / [ F2 ]³

∴ Q = [ SF6 ] / [ F2 ]³

∴ [ SF6 ] = 2 mol/L

∴ [ F2 ] = 2 mol/L

⇒ Q = ( 2 ) / ( 2³)

⇒ Q = 0.25

⇒ Q < K, reaction will make more products

 

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