Question

In a storage area of a hospital where the temperature has reached 55 °C, the pressure of oxygen gas in a 15.0-L steel cylinder is 965 Torr.What is the final pressure, in millimeters of mercury, when the temperature of the oxygen gas drops to 24 °C, and the volume and the amount of the gas do not change?

Answer 1

Answer:

$873.80\text{ mmHg}$

Explanation:

Here, we want to get the final pressure

From the pressure law, volume and temperature are directly proportinal

Mathematically:

$\frac{P_1}{T_1}\text{ = }\frac{P_2}{T_2}$

Where:

P1 is the initial pressure which is 965 torr

P2 is ?

T1 is the initial temperature which we convert to Kelvin by adding 273 K(55 + 273 = 328 k

T2 is the final temperature which is 24 + 273 = 297 K

Substituting the values, we have it that:

$\begin{gathered} \frac{965}{328}\text{ = }\frac{P_2}{297} \\ \\ P_2\text{ = }\frac{297\times965}{328}\text{ = 873.80 torr} \end{gathered}$

Now, we convert this to mmHg

Mathematically, 1 torr = 1 mmHg

We have the final pressure as 873.80 mmHg