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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

Respuesta :

Answer:

3 X ( g ) ⇄ Y ( g ) + Z ( s )

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

[tex]\frac{[Y]}{[X]^{3} }[/tex] is constant with change in initial concentration of X.

Explanation:

                                      3 X ( g ) ⇄ Y ( g ) + Z ( s )

             Equilibrium constant for the reaction is as follows

                           [tex]K_{c}[/tex] =  [tex]\frac{[Y]}{[X]^{3} }[/tex]

At equilibrium there is no change in the ratio [tex]\frac{[Y]}{[X]^{3} }[/tex] of concentration of products to reactant if initial concentration change.

Therefore  [tex]\frac{[Y]}{[X]^{3} }[/tex] is constant with change in initial concentration of X.