Question

a sealed vessel containing argon, oxygen, and nitrogen has a total pressure of 3.75 atm and partial pressures of 0.75 atm for oxygen and 1.80 atm for nitrogen. what is the partial pressure of argon in atm?

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, $P_{total} = P_{O_2} + P_{N_2} + P_{Ar}$.

Step2: Rearrange the formula

To find the partial pressure of argon ($P_{Ar}$), we rearrange the formula: $P_{Ar} = P_{total} - P_{O_2} - P_{N_2}$.

Step3: Substitute the values

Given $P_{total} = 3.75$ atm, $P_{O_2} = 0.75$ atm, and $P_{N_2} = 1.80$ atm. Substitute these into the formula: $P_{Ar} = 3.75 - 0.75 - 1.80$.

Step4: Calculate the result

First, $3.75 - 0.75 = 3.00$. Then, $3.00 - 1.80 = 1.20$.

Answer:

The partial pressure of argon is $\boldsymbol{1.20}$ atm.