A quantity of hydrogen gas occupies a volume of `30.0 mL` at a certain temperature and pressure. What volume would half of this mass of hydrogen occupy at triple the initial temperature, if the pressure was one-ninth that of the original gas?

Options

A. `270 mL`
B. `90 mL`
C. `405 mL`
D. `137 mL`

Explanation

To solve the problem, we will use the Ideal Gas Law, which states that:

\[ PV = nRT \]

Where:
- \( P \) = pressure
- \( V \) = volume
- \( n \) = number of moles
...