Question

question 21 of 30
the partial pressures of the gases in a mixture are 0.00461 atm o₂, 1.78 atm n₂, and 0.975 atm ar. what is the total pressure of the mixture?

a. 1.78 atm
b. 4.54 atm
c. 2.76 atm
d. 0.800 atm

Explanation:

Step1: Recall Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure ($P_{total}$) of a gas mixture is the sum of the partial pressures of its component gases. So, $P_{total} = P_{O_2} + P_{N_2} + P_{Ar}$.

Step2: Substitute the given partial pressures

We are given $P_{O_2} = 0.00461$ atm, $P_{N_2} = 1.78$ atm, and $P_{Ar} = 0.975$ atm. Plugging these values into the formula:

$P_{total} = 0.00461 + 1.78 + 0.975$

Step3: Perform the addition

First, add 0.00461 and 1.78: $0.00461 + 1.78 = 1.78461$

Then, add 0.975 to the result: $1.78461 + 0.975 = 2.75961 \approx 2.76$ atm.

Answer:

C. 2.76 atm