Question

A generic gas, X , is placed in a sealed glass jar and decomposes to form gaseous Y and solid Z . 3 X ( g ) − ⇀ ↽ − Y ( g ) + Z ( s ) How are these equilibrium quantities affected by the initial amount of X ( g ) placed in the container? Assume constant temperature

Answer 1

3 X ( g ) ⇄ Y ( g ) + Z ( s )

According to le chatelier principle increases in reactant concentration will shift equilibrium towrads right direction.

`([Y])/([X]^(3) )` is constant with change in initial concentration of X.

Step-by-step explanation:

3 X ( g ) ⇄ Y ( g ) + Z ( s )

Equilibrium constant for the reaction is as follows

`K_(c)` =
`([Y])/([X]^(3) )`

At equilibrium there is no change in the ratio
`([Y])/([X]^(3) )` of concentration of products to reactant if initial concentration change.

Therefore
`([Y])/([X]^(3) )` is constant with change in initial concentration of X.