HELP Pressure Change for equation without volume

In summary, the problem involves a tank initially pressurized with 5.0 atm of N2 and 10.0 atm of H2, which react to form ammonia. The partial pressure of ammonia is 3.2 atm when the reaction has reached equilibrium. Assuming constant temperature and volume, the total pressure in the tank can be calculated using the equation N2+3H2 -> 2NH3 and the given partial pressure of ammonia.
  • #1
Navygal
4
0
HELP! Pressure Change for equation without volume

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



I don't know how to go about this without using volume or number of moles. Is there another equation I should use??
Any help would be greatly appreciated
 
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  • #2


Assume the tank has volume V. You will see that the V cancels out in the end. (alternatively if you like using numbers instead of variables, just use an arbitrary volume like 1L, plug in the numbers and see what the answer is).
 
  • #3


I agree with Ygg.. Assume volume and temperature are the same at beginning and end. Then the pressure is proportional to moles. The equation is N2+3H2 -> 2NH3. Assume this has an extent of x (x moles of N2 reacted). Starting moles N2=5, H2=10. Ending moles N2=5-x, H2=10-3x, NH3=2x. Total pressure at end = sum of three partials = 15-2x.
The problem gives you NH3= 3.2 atm at end = 2x. Total pressure at end= you solve it.
 

What is the equation for calculating pressure change without volume?

The equation for calculating pressure change without volume is P1/P2 = T1/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

How does temperature affect pressure in this equation?

In this equation, temperature has a direct effect on pressure. As temperature increases, pressure also increases, and vice versa. This is because as temperature increases, the molecules in a gas move faster and collide with the walls of the container more frequently, resulting in a higher pressure.

What units should be used for pressure and temperature in this equation?

Pressure should be measured in units of pressure, such as pascals (Pa), atmospheres (atm), or torr. Temperature should be measured in units of Kelvin (K) or degrees Celsius (°C). It is important to use the same units for both initial and final values when using this equation.

Can this equation be used for any type of gas?

Yes, this equation can be used for any type of gas as long as the units for pressure and temperature are consistent. It is a general equation that applies to ideal gases, which follow the ideal gas law.

What are some practical applications of this equation?

This equation is commonly used in various scientific fields, including chemistry, physics, and engineering. It can be used to calculate pressure changes in gas systems, predict the behavior of gases under different conditions, and analyze the effects of temperature on pressure in various processes.

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