Question

The pressure of the oxygen gas inside a canister is 5.00 atm at 25.0° C. The canister is located at a camp high on Mount Everest. If the temperature at this base camp falls to - 10° what is the new pressure inside the canister?

Answer 1

To calculate the new pressure of oxygen gas when the temperature drops from 25.0°C to -10.0°C, you can use Gay-Lussac's law. After converting temperatures to Kelvins, apply the formula P1/T1 = P2/T2 to find that the new pressure is approximately 4.41 atm.

Step-by-step explanation:

The student is asking to calculate the new pressure of oxygen gas inside a canister after a temperature change from 25.0°C to -10.0°C.

This calculation involves applying Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature, assuming the volume and amount of gas are constant. To find the new pressure, we can use the formula:

P1/T1 = P2/T2,

Where P1 is the initial pressure, T1 is the initial temperature in Kelvins, P2 is the final pressure, and T2 is the final temperature in Kelvins. Converting the temperatures to Kelvins and plugging in the given values:

T1 = 25.0°C + 273.15 = 298.15 K,

T2 = -10.0°C + 273.15 = 263.15 K,

P1 = 5.00 atm,

Now we solve for P2:

P2 = P1 × (T2/T1),

P2 = 5.00 atm × (263.15 K / 298.15 K)

= 4.41 atm (approximately).

Note that we rounded the final pressure to two decimal places, assuming standard significant figures rules apply.