Question

A rigid chamber is initially filled with 4.00 atm of N2 gas and 3.00 atm of O2 gas. After these react to form N2O(g) and the chamber returns to its original temperature, the final pressure in the chamber is ?

Answer 1

The final pressure in the chamber is 5 atm.

Step-by-step explanation:

The balanced chemical reaction is:

2 N₂ (g) + O₂ (g) ⇒ 2 N₂O (g)

Initially, we have 4.00 atm of N₂ gas and 3.00 atm of O₂ gas. These are the partial pressures of each gas.

Nitrogen is the limiting reactant because it gives the fewest moles of reaction.

The initial state of the reaction is: 4.00 atm of N₂ gas and 3.00 atm of O₂

During the reaction, 4 atm of N₂ and 2 atm of O₂ are consumed to form 4 atm of N₂O

Finally, 1 atm of O₂ and 4 atm of N₂O remain

`\left[\begin{array}{cccc}&2N_2&O_2&2N_2O\\I:&4&3&-\\R:&-4&-2&+4\\F:&0&1&4\end{array}\right]`

Total Pressure of the chamber:

`P_T=P_(O_2)+P_(N_2O)`= 1 atm + 4 atm=5 atm

The final pressure in the chamber is 5 atm.