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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

Respuesta :

dsdrajlin

Answer:

2.25 atm

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.

[tex]321kPa \times \frac{1atm}{101.325kPa} = 3.17 atm[/tex]

Step 2: Convert the pressure of oxygen to atm

We will use the relationship 1 atm = 14.6959 psi.

[tex]74.0psi \times \frac{1atm}{14.6959psi} =5.04atm[/tex]

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

sebassandin

Answer:

[tex]P_H=2.25atm[/tex]

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:

[tex]P_T=P_O+P_N+P_H[/tex]

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

[tex]P_H=P_T-P_O-P_N=10.46atm-74.0psi*\frac{1atm}{14.6959psi} -321kPa*\frac{1atm}{101.325kPa} \\\\P_H=2.25atm[/tex]

Best regards.