Question

A container holds 6. 4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container. If the total pressure is 1. 24 atm. What is the partial pressure of hydrogen? Use mc032-1. Jpg. 0. 31 atm 0. 93 atm 5. 2 atm 31 atm.

Answer 1

In a mixture of gases, the total pressure is equivalent to the aggregate of all the partial pressures of the single element of the gas.

It can be written as $\rm P _{total}$ = P₁ + P₂ +  P₃ and so on.

The partial pressure will be:

Option A. 0. 31 atm

Pressure can be estimated by:

PV = nRT

$\rm P_{total} = \dfrac{n _{total }RT}{ V}$

$\rm P_{total} = \dfrac{n _{H_{2}} + n _{\rm other \;gases}}{ V}$

Where,

$\rm nH_{2} = 25\% \times n_{Total}$

And,

$\begin{aligned}\rm P_{H_{2}} &= 25\% \times \rm P_{Total}\\\\& = 25\% \times 1.24 \;\rm atm\\\\& = 1.24 \rm \;atm \times 25 \end{aligned}$

Solving finally we get,

$\rm P_{H_{2}} = 0.31 \;\rm atm$

Therefore, 0.31 atm is the partial pressure of the hydrogen gas.

To learn more about partial pressure follow the link:

brainly.com/question/1471705