A container is charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2 NH3(g)
According to Le Chatelier's Principle, an increase in pressure will shift the equilibrium to the side with fewer mols. That will be the side with NH3; therefore, additional N2 will react with additional H2 to form additional NH3.
According to Le Chatelier's principle, if the volume of a container is increased at constant temperature, the equilibrium will shift in the direction that produces more moles of gas.
In the given reaction, there are a total of 4 moles of gas on the left side (3 moles of H2 and 1 mole of N2) and 2 moles of gas on the right side (2 moles of NH3). Therefore, the reaction produces fewer moles of gas compared to the reactants.
When the volume of the container is increased, the equilibrium position will shift in the direction that generates more moles of gas to decrease the pressure. In this case, the equilibrium will shift towards the left to produce more H2 and N2, and less NH3.
So, if the volume of the container is increased at constant temperature, the amount of hydrogen, nitrogen, and ammonia gases will be altered. The system will shift towards the reactants side resulting in an increase in the concentrations of hydrogen and nitrogen, while the concentration of ammonia will decrease.
To determine what will happen if the volume of the container is increased at constant temperature, we need to understand the concept of Le Chatelier's principle. According to Le Chatelier's principle, when a system at equilibrium is subjected to a change, it will respond in a way that minimizes the effect of that change.
In this case, the system is in equilibrium with the reaction: 3H2(g) + N2(g) -> 2NH3(g). This reaction represents the production of ammonia (NH3) from hydrogen (H2) and nitrogen (N2).
When the volume of the container is increased, it means more space is available for the gases to occupy. This change affects the equilibrium because gases will tend to expand and fill the available space.
To determine the effect of the volume increase, we can analyze the stoichiometry of the reaction: 3 moles of hydrogen react with 1 mole of nitrogen to produce 2 moles of ammonia. This tells us that the reaction involves a decrease in the total number of gas molecules.
Now, by increasing the volume of the container, the system will try to compensate for the increase in volume by shifting the equilibrium in the direction that produces more gas molecules. In this case, the system will shift towards the side with a smaller number of gas molecules.
Since there are fewer gas molecules on the product side (2 moles of NH3) compared to the reactant side (3 moles of H2 and 1 mole of N2), the equilibrium will shift in the forward direction to produce more ammonia (NH3).
In summary, if the volume of the container is increased at constant temperature, the equilibrium will shift to the right, resulting in the production of more ammonia (NH3).