Question

missed this? watch kcv: amiotunt of chunge, read section 11.9. you can click on the review link to access the section in your etext a mixture of helium, nitrogen, and oxygen has a total pressure of 750 mmhg. the partial pressures of helium and nitrogen are 232 mmhg and 195 mmhg, respectively. part a what is the partial pressure of oxygen in the mixture? express your answer in millimeters of mercury to three significant figures. p(o₂) = mmhg submit request answer

Explanation:

Step1: Recall Dalton's Law

Dalton's Law states that the total pressure ($P_{total}$) of a gas mixture is the sum of the partial pressures of its components. So, $P_{total} = P_{helium} + P_{nitrogen} + P_{oxygen}$.

Step2: Rearrange the formula to solve for $P_{oxygen}$

We can rearrange the formula to $P_{oxygen} = P_{total} - P_{helium} - P_{nitrogen}$.

Step3: Substitute the given values

Given $P_{total} = 750$ mmHg, $P_{helium} = 232$ mmHg, and $P_{nitrogen} = 195$ mmHg. Substituting these values in, we get:
$P_{oxygen} = 750 - 232 - 195$

Step4: Calculate the result

First, calculate $750 - 232 = 518$. Then, $518 - 195 = 323$.

Answer:

323