The equilibrium constant for the following reaction is `1.6xx10^(5)` at `1024 K`
`H_(2)(g)+Br_(2)(g) hArr 2HBr(g)`
find the equilibrium pressure of all gases if `10.0` bar of `HBr` is introduced into a sealed container at `1024 K`.

Explanation

To solve the problem, we need to find the equilibrium pressures of all gases involved in the reaction:

\[ \text{H}_2(g) + \text{Br}_2(g) \rightleftharpoons 2 \text{HBr}(g) \]

Given:
- The equilibrium constant \( K_p = 1.6 \times 10^5 \) at \( 1024 \, K \)
- Initial pressure of \( \text{HBr} = 10.0 \, \text{bar} \)

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