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The equilibrium constant for the following reaction is \( 1.6 \times 10^{5} \) at \( 1024 \mathrm{~K} \) \( \mathrm{H}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HBr}(\mathrm{g}) \)
P
Find the equilibrium pressure of all gases if \( 10.0 \) bar of \( \mathrm{HBr} \) is introduced into a
W sealed container at \( 1024 \mathrm{~K} \).
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