A quantity of n2 gas originally held at 4.75 atm pressure in a 1.00-L container at 26c is transerred to a 10.0-L container at 20c. a quanity of o2 gas originally at 5.25 atm and 26c in a 5.00-L container is transferred to this same container. what is the total pressure in the new container

The total pressure in the new container is 5.608 atm

Explanation:

Step 1: we determine number of moles of N₂ gas present

PV = nRT

Given;

Pressure of N₂ gas = 4.75 atm

Volume of N₂ gas = 1 L

Temperature N₂ gas = 26 ⁰C

R is constant = 0.0821 atm.L/K.mol

n is the number of moles of N₂ gas = ?

Step 2: we determine number of moles of O₂ gas present

Given;

Pressure of Given;

Pressure of  O₂ gas = 5.25 atm

Volume of  O₂ gas = 5 L

Temperature N₂ gas = 20⁰C

n is the number of moles of  O₂ gas = ?

Step 3: we determine the total pressure of gases in the new container.

Total number of moles of gases = 0.1935 + 1.0912 = 1.2847

Total volume of gases = 1 + 5 = 6L

Total temperature = 26 + 20 = 46 ⁰C

Therefore, the total pressure in the new container is 5.608 atm

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