A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 and the initial pressure of chlorine was 1.65 . The piston was pushed down to change the volume to 1.00 . Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant..

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When the temperature stays the same, the volume of a gas is inversely proportional to the pressure of the gas. If a balloon is filled with 408 cubic inches of a gas at a pressure of 14 pounds per square inch, find the new pressure of the gas if the volume is decreased to 68 cubic inches

To calculate the final pressure of the gas, we can use Boyle's Law, which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume at constant temperature and number of moles.

Boyle's Law can be expressed as:

P1 * V1 = P2 * V2

Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume

In this case, we have:
P1 = 1.65 atm
V1 = 3.00 L
V2 = 1.00 L

We need to solve for P2, the final pressure.

Rearranging the equation, we get:

P2 = (P1 * V1) / V2

Substituting the given values, we get:

P2 = (1.65 atm * 3.00 L) / 1.00 L

P2 = 4.95 atm

Therefore, the final pressure of the gas is 4.95 atm.