Consider the following reaction: NH4HS( s )NH3( g )+H2S( g ) An equilibrium mixt

Question

Consider the following reaction:
NH4HS(s)NH3(g)+H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.288 Mand [H2S]= 0.350 M .

Part A

What is the value of the equilibrium constant (Kc) at this temperature?

Consider the following reaction:
NH4HS(s)NH3(g)+H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.288 Mand [H2S]= 0.350 M .

Part A

What is the value of the equilibrium constant (Kc) at this temperature?

Explanation / Answer

NH4HS(s)      NH3(g)+H2S(g)
Given the equilibrium concentration of [NH3] = 0.288 M

                                                and [H2S] = 0.350 M

The equilibrium constnat of the above reaction is Kc = ( [NH3(g)][H2S(g) ] ) / ([NH4HS(s) ])

But at equilibrium the concentration of solids will not effect the equilibrium constant , so [NH4HS(s) ]=1

Then Kc = [NH3(g)][H2S(g) ]

      = 0.288 M x 0.350 M

= 0.101 M2

Therefore the value of the equilibrium constant (Kc) at this temperature is 0.101

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