Let's break down the problem step by step:
1. Conversion of total pressure:
The total pressure given is in atmospheres (atm). We need to convert this pressure to torr since the partial pressure of helium is given in torr and we need consistency in units. The conversion factor between atm and torr is 1 atm = 760 torr.
[tex]\[
\text{Total pressure in torr} = 2.73 \, \text{atm} \times 760 \, \text{torr/atm}
\][/tex]
[tex]\[
\text{Total pressure in torr} = 2.73 \times 760
\][/tex]
[tex]\[
\text{Total pressure in torr} = 2074.8 \, \text{torr}
\][/tex]
2. Calculating the pressure of hydrogen in torr:
The total pressure is the sum of the partial pressures of helium and hydrogen. Therefore, we can calculate the pressure of hydrogen by subtracting the pressure of helium from the total pressure.
[tex]\[
\text{Pressure of hydrogen in torr} = \text{Total pressure in torr} - \text{Pressure of helium in torr}
\][/tex]
[tex]\[
\text{Pressure of hydrogen in torr} = 2074.8 \, \text{torr} - 766.6 \, \text{torr}
\][/tex]
[tex]\[
\text{Pressure of hydrogen in torr} = 1308.2 \, \text{torr}
\][/tex]
3. Conversion to mmHg:
Since 1 torr is exactly equal to 1 mmHg, the pressure in torr is numerically equal to the pressure in mmHg.
[tex]\[
\text{Pressure of hydrogen in mmHg} = 1308.2 \, \text{mmHg}
\][/tex]
4. Rounding to one decimal place:
The calculated pressure is already to one decimal place.
So, the pressure of hydrogen is:
[tex]\[
\boxed{1308.2 \, \text{mmHg}}
\][/tex]
