Question

1 point

A container with nitrogen, oxygen, and hydrogen has a pressure of 10.46
atm. If the pressure of nitrogen is 321 kPa and the pressure of oxygen is
74.0 psi, what is the pressure of hydrogen? *
2.25 atm
18.7 atm
4.90 atm
237 atm

Answer 1

`P_H=2.25atm`

Step-by-step explanation:

Hello,

IN this case, we can apply the Dalton's law in order to understand the pressure behavior of a mixture as the summation of all the pressures of the compounds in the mixture, in this case, nitrogen, oxygen and hydrogen:

`P_T=P_O+P_N+P_H`

So, since we are asked to compute the pressure of hydrogen, we simply solve for it:

`P_H=P_T-P_O-P_N=10.46atm-74.0psi*(1atm)/(14.6959psi) -321kPa*(1atm)/(101.325kPa) \\\\P_H=2.25atm`

Best regards.

Answer 2

2.25 atm

Step-by-step explanation:

Given data

• Pressure of N₂: 321 kPa

• Pressure of O₂: 74.0 psi

• Pressure of H₂: ?

• Total pressure: 10.46 atm

Step 1: Convert the pressure of nitrogen to atm

We will use the relationship 1 atm = 101.325 kPa.

`321kPa * (1atm)/(101.325kPa) = 3.17 atm`

Step 2: Convert the pressure of oxygen to atm

We will use the relationship 1 atm = 14.6959 psi.

`74.0psi * (1atm)/(14.6959psi) =5.04atm`

Step 3: Calculate the partial pressure of hydrogen

The total pressure is the sum of the partial pressures.

P = pN₂ + pO₂ + pH₂

pH₂ = P - pN₂ - pO₂

pH₂ = 10.46 atm - 3.17 atm - 5.04 atm

pH₂ = 2.25 atm