Consider the reaction:NH4HS(s) ∆ NH3( g) + H2S( g)At a certain temperature, Kc = 8.5 * 10 - 3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

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Asked Oct 18, 2019
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Consider the reaction:
NH4HS(s) ∆ NH3( g) + H2S( g)

At a certain temperature, Kc = 8.5 * 10 - 3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

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Expert Answer

Step 1

A reversible chemical reaction can move in either forward or backward direction. The stage of a reversible reaction at which the rate of forward and backward reaction become equal to each other is called an equilibrium stage.

Step 2

An equilibrium reaction can be defined with the help of equilibrium constant that is the ratio of concentration of product and reactant at equilibrium stage.

Step 3

The reaction quotient is also ratio of concentration of product and reactant at any other stage of the revers...

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>NH) +HS) NH,HS [NH HS) Qc = - ΝΗ, (s) 3( g) 3( g) =[NH) ] [H,S] 1 NH HS Kc (g) =[NH5( B} 1

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