Question

If a sample of gas at 37.1 oC and 717 torr occupies 18.1 L of space, then what would be the pressure (in torr) of the gas if the temperature drops to 10.5 oC and volume increases to 37 L?

Answer 1

The final pressure of the gas would be 697.6 torr.

Step-by-step explanation:

To solve this problem, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

Where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature of the gas.

Plugging in the given values:

P1 = 717 torr, V1 = 18.1 L, T1 = 37.1°C = 37.1 + 273.15 = 310.25 K

P2 is the unknown, V2 = 37 L, and T2 = 10.5°C = 10.5 + 273.15 = 283.65 K

Substituting these values into the combined gas law equation:

717 * 18.1 / 310.25 = P2 * 37 / 283.65

Solving for P2:

P2 = (717 * 18.1 * 283.65) / (310.25 * 37)

P2 = 697.6 torr

The final pressure of the gas would be 697.6 torr.