In part D of task 1, you identified at least two ways in which the reaction of nitrogen and hydrogen could be changed to alter the equilibrium. Use the simulation to test those changes. Describe how you used the simulation to model the changes and the results they produced. Use these methods if you find them helpful:
Look at the pie graph to see how the system changes.
Use the Temperature slider at the bottom to cool or heat the mixture.
Click the pause button on the simulation to observe the number of particles at any point of time.
Honestly I just need a random answer that seems reasonable enough
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Results of the experiment:
- Both the reactant gas and the product gas are in the same phase equilibrium with the same number of species present. Thus, the change in pressure has no impact.
- The quantity of the product will increase as the pressure rises. In order to counterbalance the change and lower the pressure, the equilibrium will move to the right, where there are less molecules. The reaction is exothermic, which means it produces heat by having a negative enthalpy change. The product's volume will shrink. The equilibrium will shift left in an endothermic direction to chill the reaction and reduce the amount of ammonia that is produced.
- If the reaction is in equilibrium, the catalyst will simply cause it to proceed more quickly in both directions without changing the rate at which the product is produced.
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