For the following reaction, Kp = 1.9 ✕ 104 at 1722 K. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) What is the value of Kp for the following reactions at 1722 K? (a) HBr(g) equilibrium reaction arrow 1/2 H2(g) + 1/2 Br2(g)

The value of equilibrium constant for the given reaction is,

Explanation:

The given chemical equation is:

;

We need to calculate the equilibrium constant for the chemical equation, which is:

;

If the equation is revered then the equilibrium constant will be the reciprocal of the reaction.

If the equation is half then the equilibrium constant will be square-root of the reaction.

The value of equilibrium constant for the given reaction is:

Hence, the value of equilibrium constant for the given reaction is,

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.