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ammonia reacts with oxygen according to the following equation. 4 nh3(g) 5 o2(g) equilibrium reaction arrow 4 no(g) 6 h2o(g) the enthalpy of reaction for this reaction is negative. identify two changes that could be made to the system to shift the equilibrium toward the products and two changes that could be made to shift the equilibrium toward the reactants. (select all that apply.) changes that would shift the equilibrium toward the products: increasing the volume of the system increasing the concentration of no or h2o decreasing the concentration of nh3 or o2 reducing the temperature of the system changes that would shift the equilibrium toward the reactants: increasing the volume of the system increasing the concentration of no or h2o decreasing the concentration of nh3 or o2 reducing the temperature of the system

Respuesta :

Based on the number of particles involved and the enthalpy of the reaction, changes that would shift the equilibrium to the right would, according to Le Chatelier's principle, include increasing the volume of the system, reducing the pressure of the system, reducing the temperature of the system, increasing the concentration of ammonia and/or oxygen and reducing the concentration of NO and/or water. Changes in the opposite direction would cause the equilibrium to shift towards the reactants.

Upon increasing pressure or reducing volume, the equilibrium shifts in the direction that produces fewer gaseous particles. In this case, that's the reactants (9 molecules) and not the products (10 molecules). When considering temperature, it is useful to consider heat as one of the reaction components. When the enthalpy of the reaction is negative, heat is produced so it can be considered to be one of the products. Le Chatelier's principle states that upon changing one of the variables, the equilibrium will shift in the direction that counteracts the effects of the change. So, when reducing the temperature of the system, we are taking the heat out of the system, so equilibrium will shift to the products so that it can produce more heat, and vice versa. The same principle applies to the concentrations of ammonia, oxygen, water, and NO.

You can learn more about Le Chatelier's principle here:
brainly.com/question/2001993

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