7.27. The equilibrium constant for the following reaction is 1.6 ×105 at 1024K
H2(g) + Br2(g) ⇌ 2HBr(g)
Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024K.
7.27. The equilibrium constant for the following reaction is 1.6 ×105 at 1024K
H2(g) + Br2(g) ⇌ 2HBr(g)
Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024K.
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1 Answer
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For the equilibrium reaction
2HBr (g) ? H2(g) + Br2(g) , the equilibrium constant is K = 1/1.6×105.
Initial pressure 10 0 0
At equilibrium 10-p p/2 p/2
The equilibrium consta...more
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