I am given the following reaction:
2NH3(g) -----> N2(g) + 3H2(g)
6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium mixture has 4.2 mols of nitrogen, what is the value of the equilibrium constantsupposed to be?
My question is, how do I arrive at the following in my answer:
[N2] = 2.7 moles in 2.2l = 1.22 moles/liter
Where did the 2.7 moles come from?
If the reaction went to completion, the 6.4 mols of NH3 would produce 3.2 mols of N2 and three times as many of H2. I don't see how 4.2 mols of N2 could be formed. I also don't see where the 2.7 moles came from. Have you stated all numbers of the problem correctly?
To understand where the value of 2.7 moles comes from, let's analyze the given reaction and the given information step by step.
The balanced equation for the reaction is:
2 NH3(g) -----> N2(g) + 3 H2(g)
The reaction tells us that 2 moles of ammonia gas (NH3) react to form 1 mole of nitrogen gas (N2) and 3 moles of hydrogen gas (H2).
In the given question, we are given information about the initial number of moles of ammonia gas (NH3), which is 6.4 moles, and the volume of the flask, which is 1.7 liters. We are also told that at equilibrium, the mixture has 4.2 moles of nitrogen gas (N2).
To find the equilibrium constant, we need to calculate the concentrations of each species at equilibrium. Concentration is typically expressed in moles per liter (mol/L).
For nitrogen gas (N2), we are given the equilibrium value.
[N2] = 4.2 moles in 1.7 L = 2.47 moles/liter (rounded to 2 decimal places)
Now, let's calculate the concentration of ammonia gas (NH3).
At the start, the number of moles of ammonia gas was 6.4 moles in 1.7 liters, which gives us:
[NH3] = 6.4 moles/1.7 L = 3.76 moles/liter (rounded to 2 decimal places)
Since 2 moles of ammonia react to form 1 mole of nitrogen gas, we can divide the concentration of NH3 by 2 to find the concentration of N2:
[N2] = [NH3]/2
[N2] = 3.76 moles/liter / 2 = 1.88 moles/liter (rounded to 2 decimal places)
Therefore, the correct concentration of nitrogen gas (N2) at equilibrium should be 1.88 moles/liter, not 2.7 moles/liter as mentioned in your answer. It appears that there may have been a calculation error in your solution or a misunderstanding.