Sure! Let's break down the problem step by step.
1. Understand the Problem:
- We have a 20.0-liter flask containing a mixture of gases.
- The components are Argon and Oxygen.
- The pressure of Argon in the flask is 0.72 atmospheres.
- The pressure of Oxygen in the flask is 1.65 atmospheres.
- We need to find the total pressure in the flask and select from the given choices.
2. Relevant Concept:
- According to Dalton's Law of Partial Pressures, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of individual gases.
- Mathematically, [tex]\( P_{\text{total}} = P_{\text{argon}} + P_{\text{oxygen}} \)[/tex].
3. Calculate the Total Pressure:
[tex]\[
P_{\text{total}} = P_{\text{argon}} + P_{\text{oxygen}}
\][/tex]
Given:
[tex]\[
P_{\text{argon}} = 0.72 \text{ atm}
\][/tex]
[tex]\[
P_{\text{oxygen}} = 1.65 \text{ atm}
\][/tex]
[tex]\[
P_{\text{total}} = 0.72 \text{ atm} + 1.65 \text{ atm}
\][/tex]
[tex]\[
P_{\text{total}} = 2.37 \text{ atm}
\][/tex]
4. Compare with Choices:
- A. [tex]\(0.93 \text{ atm}\)[/tex]
- B. [tex]\(2.37 \text{ atm}\)[/tex]
- C. [tex]\(8.44 \text{ atm}\)[/tex]
- D. [tex]\(18.6 \text{ atm}\)[/tex]
5. Select the Correct Choice:
- The total pressure calculated is [tex]\(2.37 \text{ atm}\)[/tex].
- Therefore, the correct choice is B. [tex]\(2.37 \text{ atm}\)[/tex].
So, the total pressure in the flask is [tex]\(2.37 \text{ atm}\)[/tex], and the correct answer is B.
