When a container is filled with 3.00 moles of $H_2$, 2.00 moles of $O_2$, and 1.00 mole of $N_2$, the pressure in thecontainer is 768 kPa. What is the partial pressure of $O_2$?

Md Ariful Islam

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Md Ariful Islam

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Partial Pressure of $O_2$ = 256 kPa.

Dalton's law of partial pressures covers two concepts;

  • Mole fraction
  • Partial pressure

Let's talk about Mole Fraction first.

You have a mixture of $H_2$, $O_2$ and $N_2$ in the container. The mole fraction of gas $O_2$ is worked out by dividing the number of moles of gas $O_2$ by the total number of moles of gas.

$chi_(O_2) = ("number of moles of gas" O_2)/("total number of moles of gas")$

$chi_(O_2) = (2cancel("moles"))/((3+2+1)cancel("moles")) = 1/3$

Next, the equation of the partial pressure of a gas can be written as;

$P_(O_2) = "mole fraction of " O_2 xx "Total Pressure"$

Since now we know the mole fraction of $O_2$, and the total pressure, we can just substitute the values into the partial pressure equation.

$P_(O_2) = 1/3 * "768 kPa" = "256 kPa"$

Note:

The total pressure can be calculated using this;

$P_"total" = P_"gas A" + P_"gas B" + P_"gas C" +...$

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