A 20.0-liter flask contains a mixture of argon at 0.72 atmosphere and oxygen at 1.65 atmospheres. What is the total pressure in the flask?

A. 0.93 atm
B. 2.37 atm
C. 8.44 atm
D. 18.6 atm



Answer :

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.