A 4.0 L of a gas at a pressure of 205 kPa is allowed to expand to a volume of 16.0 L. Calculate the pressure in atmospheres (atm) in the container at constant temperature.

Answer 1

To solve this problem, we can use the formula for the ideal gas law:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.

Since the temperature is constant, we can simplify the equation to:

P1V1 = P2V2

Where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.

Substituting the given values, we get:

205 kPa x 4.0 L = P2 x 16.0 L

Simplifying the equation, we get:

P2 = (205 kPa x 4.0 L) / 16.0 L

P2 = 51.25 kPa

To convert this to atmospheres, we divide by the standard atmospheric pressure (101.3 kPa):

P2 = 51.25 kPa / 101.3 kPa/atm

P2 = 0.506 atm (rounded to three significant figures)

Therefore, the pressure in the container at constant temperature is 0.506 atm.