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 1.30atm . 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

Use P1V1=P2V2

Since you don't know the P2 just plug in all of the known factors:

(3.00L)(1.30atm)= (1.00L)P2

Solve for P2

3.90=1

P2=3.90atm

To solve this problem, we can use Boyle's Law, which states that the product of pressure and volume is constant when temperature and moles of gas remain constant.

Boyle's Law Equation: P1V1 = P2V2

Given:
Initial Volume (V1) = 3.00 L
Initial Pressure (P1) = 1.30 atm
Final Volume (V2) = 1.00 L

We need to find the final pressure (P2).

Using Boyle's Law Equation:

P1V1 = P2V2

Substituting the given values:

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

Rearranging the equation to solve for P2:

P2 = (P1V1) / V2

P2 = (1.30 atm * 3.00 L) / 1.00 L

P2 = 3.90 atm

Therefore, the final pressure of the gas is 3.90 atm.