Question

Helium occupies 293 mL at 788 Torr and 25C. If the sample is condensed into a 0.115 liter flask, what will the new pressure be, assuming constant temperature?

Answer 1

=2007.69 Torr

Step-by-step explanation:

The new pressure of helium gas assuming constant temperature is equal to 2007.69

Torr.

Given the following data:

Initial volume = 293 mL

Final volume = 0.115 L

Initial pressure = 788 Torr

Temperature = 25°C.

Conversion:

Initial volume = 293 mL to L = 293/1000=0.293L

To determine the new pressure assuming constant temperature, we would apply Boyle's law:

Mathematically, Boyle's law is given by the formula;

PV=K

P1V1=P2V2

Where;

P1 is the original (initial) pressure.

P2 is the final pressure.

V1 is the original (initial) volume.

V2 is the final volume.

Substituting the given parameters into the formula, we have;

788×0.293 = P2 × 0.115

230.884 = 0.115P2

P2 = 230.884/0.115

P2 =2007.69