\begin{tabular}{|l|l|}
\hline
Ideal gas law & [tex]$P V=n R T$[/tex] \\
\hline
& [tex]$R=8.314 \frac{L \cdot kPa}{mol \cdot K}$[/tex] \\
Ideal gas constant & or \\
& [tex]$R=0.0821 \frac{L \cdot atm}{mol \cdot K}$[/tex] \\
\hline
Standard atmospheric pressure & [tex]$1 atm = 101.3 kPa$[/tex] \\
\hline
Celsius to Kelvin conversion & [tex]$K = {}^{\circ}C + 273.15$[/tex] \\
\hline
\end{tabular}

When a chemist collects hydrogen gas over water, she ends up with a mixture of hydrogen and water vapor in her collecting bottle. If the pressure in the collecting bottle is 97.1 kilopascals and the vapor pressure of the water is 3.2 kilopascals, what is the partial pressure of the hydrogen?

A. [tex]$93.9 \, kPa$[/tex]
B. [tex]$98.1 \, kPa$[/tex]
C. [tex]$100.3 \, kPa$[/tex]
D. [tex]$104.5 \, kPa$[/tex]

To find the partial pressure of hydrogen gas in the collecting bottle, we can follow these steps:

1. Understand the Given Information:
- The total pressure in the collecting bottle is 97.1 kilopascals [tex]$kPa$[/tex].
- The vapor pressure of the water is 3.2 kilopascals [tex]$kPa$[/tex].

2. Concept of Partial Pressure:
- The total pressure in a gas mixture is the sum of the partial pressures of each component gas.
- In this scenario, the total pressure is the sum of the partial pressures of hydrogen gas and water vapor.

3. Calculate the Partial Pressure of Hydrogen:
- To find the partial pressure of the hydrogen gas, we subtract the vapor pressure of the water from the total pressure.
[tex]\[
\text{Partial Pressure of Hydrogen} = \text{Total Pressure} - \text{Vapor Pressure of Water}
\][/tex]
[tex]\[
\text{Partial Pressure of Hydrogen} = 97.1\, kPa - 3.2\, kPa = 93.9\, kPa
\][/tex]

4. Select the Correct Answer:
- The partial pressure of hydrogen is calculated to be 93.9 kilopascals.
- Therefore, the correct answer is [tex]$ \boxed{93.9\, kPa} $[/tex].