Question

A box with a volume of 11.2 L contains 1.0 mol of nitrogen and 2.0 mol of hydrogen at 0°C which of the following statements is true?

R = 8.31 kPa x L/mol x K, PV = nRT

a. The partial pressures of N₂ and H₂ are equal.
b. The partial pressure of N₂ is 202 kPa.
c. The total pressure is 303 kPa.
d. The total pressure in the box is 202 kPa.

Answer 1

Hope this helps you.

Answer 2

Answer: b. The partial pressure of N₂ is 202 kPa.

Step-by-step explanation:

According to the ideal gas equation:'

`PV=nRT`

Pressure of the gas = ?

Volume of the gas = 11.2 L

Temperature of the gas = 0°C = 273K(0°C = 273 K)

Value of gas constant R=8.314 kPaL\Kmol

n = moles of gas = 3.0

`P=(nRT)/(V)=(3* 8.314* 273)/(11.2)=607kPa`

`p_(N_2)=x_(N_2)* P`

`x_(N_2)` = mole fraction=
`\frac{\text {moles of}{N_2}}{\text {total moles}}=(1)/(3)=0.33`

`p_(N_2)=0.33* 607=202kPa`

`p_(H_2)=x_(H_2)* P`

`x_(H_2)` = mole fraction=
`\frac{\text {moles of}{H_2}}{\text {total moles}}=(2)/(3)=0.67`

`p_(H_2)=0.67* 607=405kPa`