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 and the initial pressure of chlorine was 1.15 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..
Pfinal= ?? atm
P1V1=P2V2
i worked this one out and got 0.383...
ok forget it i mixed up v initial and v final, i got the correct answer now...3.45
To calculate the final pressure of the gas, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature and number of moles. Boyle's Law is expressed as:
P1 * V1 = P2 * V2
where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
Given:
Initial volume, V1 = 3.00 L
Initial pressure, P1 = 1.15 atm
Final volume, V2 = 1.00 L
Number of moles (which remains constant) = n
Using Boyle's Law, we can rearrange the equation to solve for P2 (final pressure):
P2 = (P1 * V1) / V2
Substituting the given values into the equation:
P2 = (1.15 atm * 3.00 L) / 1.00 L
Calculating this expression:
P2 = 3.45 atm
Therefore, the final pressure of the gas is 3.45 atm.