Question

A sample of three mixed gases is at 630.0 mmHg. If the partial pressure of

CO2 is 124.0 mmHg and the partial pressure of N2 is 160.0 mmHg, what is the

partial pressure of O2? *

A-914.0 mmHg

B-346.0 mmHg

C-284.0 mmHg

D-46.0 mmHg

Answer 1

B-346.0 mmHg.

Step-by-step explanation:

Hi there!

In this case, according to the Dalton's law, which explains that the total pressure of a gas mixture is calculated by adding up the partial pressure of each gas, we can set up the following equation for the mixture given here:

`P_T=p_(CO_2)+p_(N_2)+p_(O_2)`

In such a way, for the required answer, it solve for the partial pressure of oxygen to obtain:

`p_(O_2)=P_T-p_(CO_2)-p_(N_2)`

Thereafter, we plug in the known pressures to obtain:

`p_(O_2)=630mmHg-124mmHg-160mmHg\\\\p_(O_2)=346mmHg`

And the answer is B-346.0 mmHg.

Best regards!