The equilibrium constant for the following reaction is1.6\times 10^5 a – InterviewSolution

1.	The equilibrium constant for the following reaction is1.6\times 10^5 at 1024 K. 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 1024 K.
Answer» The equilibrium constant for the following reaction is1.6\times 10^5 at 1024 K. $H_{2} (g) + B r_{2} (g) \leftrightarrow 2 H B r (g)$ Find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K.

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