A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 L

Question

and the initial pressure of chlorine was 1.70 atm
. The piston was pushed down to change the volume to 1.00 L
. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.

Answer 1

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

PV = nRT

where
P = pressure
V = volume
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature

Since the number of moles and the temperature remain constant, we can simplify the equation to:

P1V1 = P2V2

Where
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume

Plugging in the known values:

(1.70 atm)(3.00 L) = P2(1.00 L)

5.10 atm = P2(1.00 L)

P2 = 5.10 atm

Therefore, the final pressure of the gas is 5.10 atm.