Question

A recently filled 4.60 L gas cylinder has a pressure of 212 atm at room temp (25 degrees C). At what temp. would the gas reach the potentially dangerous pressure of 2.28 x 10^5 toss?

Answer 1

A recently filled 4.60 L gas cylinder has a pressure of 212 atm at room temp (25 degrees C). At what temp. would the gas reach the potentially dangerous pressure of 2.28 x 10^5 torr?

Solution:

Gas will be really dangerous when its volume is closer to the volume of a cylinder, that is, the value of 4.60 L.

We calculate the temperature of gas by Gay-Lussac's law: $\frac{P_1}{P_2} = \frac{T_1}{T_2}$ , where $P$ - pressure, atm., $T$ - temperature, K, V-const.

We convert the pressure from torr to atm. As we know, the torr is defined as $\frac{1}{760}$ atm. exactly. So, the $2.28 \cdot 10^5$ torr is equal to $2.28 \cdot 10^5 / 760 = 300$ atm.

$$T _ {2} = \frac {3 0 0 \cdot 2 9 8}{2 1 2} = 4 2 1 K \text{ or } 1 4 8. 7 ^ {\circ} C.$$

Answer:

The temperature of gas is $148.7^{\circ}\mathrm{C}$ .