Stuck on Change in pressure after reaction

[Navygal]

Homework Statement

A tank is pressurized with 5.0 atm of N2 and 10.0 atm of H2. Ammonia (NH3) is formed. When the pressure finally remains constant, indicating that the reaction has proceeded as far as it will go, the partial pressure of ammonia is 3.2 atm. What is the total pressure in the tank assuming that neither the temperature nor the volume of the container have changed?

Homework Equations

PV=nRT

The Attempt at a Solution

The only equations I can think to use require moles or volumes, neither of which is given.
I'm stuck, please help

 

[anathema]

!

Thank you for posting your question. It seems that you are trying to solve for the total pressure in a tank after a reaction has occurred. In order to solve this problem, we can use the ideal gas law, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

In this case, we know that the temperature and volume of the container have not changed, so we can assume that T and V are constant. We also know the partial pressure of ammonia (3.2 atm) and the initial pressures of N2 (5.0 atm) and H2 (10.0 atm). We can set up the equation as follows:

(5.0 atm + 10.0 atm + 3.2 atm) = nRT

Since we are assuming that the temperature and volume have not changed, we can simplify this equation to:

18.2 atm = nRT

Now, we need to find the number of moles of ammonia in the tank. We can use the ideal gas law again to solve for n:

PV = nRT

(3.2 atm)(V) = nRT

Solving for n, we get:

n = (3.2 atm)(V)/RT

Now, we can substitute this value for n in our first equation:

18.2 atm = [(3.2 atm)(V)/RT]RT

Simplifying this equation, we get:

18.2 atm = 3.2 atm(V)

Solving for V, we get:

V = 18.2 atm/3.2 atm = 5.6875 L

Therefore, the total pressure in the tank is 18.2 atm, assuming that neither the temperature nor the volume of the container have changed.

I hope this helps you solve the problem. Let me know if you have any further questions. Good luck with your studies!

Scientist

 

[kerimek]

!

One possible approach to solving this problem is to use the ideal gas law, PV=nRT, to calculate the number of moles of each gas present before and after the reaction. From there, you can use the balanced chemical equation to determine the moles of ammonia formed and the resulting partial pressure. Then, using the total number of moles and the known total volume of the tank, you can calculate the total pressure in the tank using the ideal gas law. Another approach could be to use Dalton's law of partial pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas. In this case, you would use the partial pressure of ammonia and the known partial pressures of nitrogen and hydrogen to calculate the total pressure in the tank. Both of these methods require some additional information, such as the volume of the tank and the temperature, which may need to be given or assumed in order to solve the problem. It may also be helpful to draw a diagram and label the initial and final pressures in the tank to better visualize the problem.