Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The decomposition of NH4HS

NH4HS(s) ⇄ NH3(g) + H2S(g)

is an endothermic process. Using Le Chatelier’s principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?

Interpretation Introduction

Interpretation: The effect of the given changes on the position of the equilibrium of given reaction has to be explained using Le Chatelier’s principle.

Concept introduction:

  • Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved when the concentrations of reactants and products become constant.
  • Concentration =AmountofsubstanceVolume
  • Le Chatelier’s principle states that if a system in chemical equilibrium is subjected to a disturbance (in concentration, pressure, and temperature) it tends to change in a way that opposes this disturbance.
  • Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions. Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.
  • In an endothermic reaction there is a net abortion of energy.

The decomposition of NH4HS is an endothermic reaction, the balanced equation for this reaction is,


The changes in various factors and its effect on to the equilibrium of the reaction can be explained using Le Chatelier’s principle as follows,

  • Increasing the temperature

The given reaction is an endothermic reaction. That means energy will be absorbed in this reaction which results in the decline of temperature.

Forward reaction is favored by absorption of energy.  If the temperature of the system increase and the system will tends to reduce this change in accordance with the Le Chatelier’s principle. Therefore this change will shift the reaction equilibrium on to the forward direction.

  • Addition of more NH4HS

According with Le Chatelier’s principle, the addition of more NH4HS disturbs the equilibrium

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