A mixture of gases with a total pressure of 97.8 kPa contains helium, argon, and krypton. The partial pressure of krypton is 14 kPa, and the partial pressure of helium is 48 kPa. What is the partial pressure of argon?

Sure! Let's solve the problem step by step:

1. Understand the problem:
- We have a mixture of gases (helium, argon, and krypton) with a total pressure of 97.8 kPa.
- We're given the partial pressure of krypton as 14 kPa.
- We're also given the partial pressure of helium as 48 kPa.
- We need to find the partial pressure of argon.

2. Use Dalton's Law of Partial Pressures:
- According to Dalton’s Law, the total pressure of a mixture of gases is the sum of the partial pressures of each individual gas.
- The formula is:
[tex]\[
\text{Total Pressure} = \text{Pressure of Helium} + \text{Pressure of Krypton} + \text{Pressure of Argon}
\][/tex]

3. Set up the equation:
- Given:
[tex]\[
\text{Total Pressure} = 97.8 \, \text{kPa}
\][/tex]
[tex]\[
\text{Pressure of Helium} = 48 \, \text{kPa}
\][/tex]
[tex]\[
\text{Pressure of Krypton} = 14 \, \text{kPa}
\][/tex]
- We need to find the Pressure of Argon:
[tex]\[
\text{Pressure of Argon} = \text{Total Pressure} - (\text{Pressure of Helium} + \text{Pressure of Krypton})
\][/tex]

4. Calculate the partial pressure of argon:
- Substitute the given values into the equation:
[tex]\[
\text{Pressure of Argon} = 97.8 \, \text{kPa} - (48 \, \text{kPa} + 14 \, \text{kPa})
\][/tex]
- Simplify the equation:
[tex]\[
\text{Pressure of Argon} = 97.8 \, \text{kPa} - 62 \, \text{kPa}
\][/tex]
[tex]\[
\text{Pressure of Argon} = 35.8 \, \text{kPa}
\][/tex]

Therefore, the partial pressure of argon is 35.8 kPa.