Question

what is the partial pressure of each gas in a 26L container at 27°c that holds 5 moles of carbon dioxide,3.3 moles of nitrogen and 1.5 moles of hydrogen, and has a total pressure of 1.05

Answer 1

pCO₂ = 0.54 atm

pN₂ = 0.35 atm

pH₂ = 0.16 atm

Step-by-step explanation:

Step 1: Calculate the total number of gaseous moles

The total number of gaseous moles (n) is equal to the sum of the moles of the individual gases.

n = nCO₂ + nN₂ + nH₂ = 5 mol + 3.3 mol + 1.5 mol = 9.8 mol

Step 2: Calculate the partial pressure of each gas

We will use the following expression.

pi = P × χi

where,

pi: partial pressure of the gas i

P: total pressure (1.05 atm)

χi: mole fraction of the gas i

pCO₂ = 1.05 atm × (5 mol/9.8 mol) = 0.54 atm

pN₂ = 1.05 atm × (3.3 mol/9.8 mol) = 0.35 atm

pH₂ = 1.05 atm × (1.5 mol/9.8 mol) = 0.16 atm