How will the equilibrium position of a gas- phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
Answer to relevant QuestionsSuppose the reaction system UO2(s) + 4HF(g) ⇌ UF4(g) + 2H2O(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will ...Hydrogen for use in ammonia production is produced by the reaction What will happen to a reaction mixture at equilibrium if a. H2O(g) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert ...An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature as follows: 3H2(g) + N2(g) ⇌ 2NH3(g) At equilibrium, the concentrations are [H2] = 5.0 M, [N2] = 8.0 M, and [NH3] ...For the reaction NH3(g) + H2S(g) ⇌ NH4HS(s) K = 400. at 35.0oC. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00- L vessel, what mass of NH4HS will be present at equilibrium? What is the pres-sure of H2S at ...A mixture of N2, H2 and NH3 is at equilibrium according to the equation N2(g) + 3H2(g) ⇌ 2NH3(g) as depicted below. The volume is suddenly decreased (by increasing the external pressure), and a new equilibrium is ...
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