What pressure would have to be applied to a 27.2-mL
sample of gas at 25 °C and 1.00 atm to compress its
volume to 1.00 mL without a change in temperature?

27.2atm

Explanation:

Data obtained from the question include:

V1 (initial volume) = 27.2mL

P1 (initial Pressure) = 1atm

V2 (final volume) = 1mL

P2 (final pressure) =?

Since the temperature is constant, the gas is obeying Boyle's law.

Mathematically, Boyle's law is expressed as:

P1V1 = P2V2

1 x 27.2 = P2 x 1

P2 = 27.2atm

The final pressure is 27.2atm.

Therefore, the pressure needed to compress the gas is 27.2atm

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa