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,

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.