Question

The enclosed cabin of a submarine has a volume of 2.4 × 105 liters, a temperature of 312 K, and a pressure of 116 kPa. As people in the cabin breathe, carbon dioxide gas, CO2(g), can build up to unsafe levels. Air in the cabin becomes unsafe to breathe when the mass of CO2(g) in this cabin exceeds 2156 grams. Show a numerical setup for calculating the pressure in the submarine cabin if the cabin temperature changes to 293 K

Answer 1

Answer:

$P_2=108.9kPa$

Explanation:

Hello,

In this case, we are noticing a change in the cabin's temperature, therefore, temperature is the only changing variable in addition to the pressure as the cabin is rigid so its volume does not change. Additionally, we do not know the rate at which the mass varies, thus, we simply use Gay-Lussac's to compute the pressure at the second state temperature as shown below:

$P_1T_2=P_2T_1\\P_2=\frac{P_1T_2}{T_1}=\frac{116kPa*293K}{312K}\\P_2=108.9kPa$

Best regards.

Answer 2

• Gay-Lussac's Law states that the pressure of a given mass of gas varies directly with the absolute temperature of the gas, when the volume is kept constant.
• Temperature also illustrates a direct relationship. As a gas is cooled at constant volume, its pressure continually decreases until the gas condenses to a liquid.

In the given question, we are noticing a change in the cabin's temperature, therefore, temperature is the only changing variable in addition to the pressure as the cabin is rigid so its volume does not change.

Additionally, we do not know the rate at which the mass varies, thus, we simply use Gay-Lussac's to compute the pressure at the second state temperature as shown below:

$P_1T_2=P_2T_1\\\\P_2=\frac{P_1T_2}{T_1} \\\\P_2=108.9kPa$

Thus this represents the relationship.

Learn more:

brainly.com/question/23830485