Question

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 1.60 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

Using Boyle's Law, the final pressure of chlorine gas compressed from 3.00 L to 1.00 L is calculated to be 4.80 atm, assuming constant temperature and amount of gas.

Step-by-step explanation:

The problem presented involves a chlorine gas sample compressed in a cylinder with a piston. The volume of the chlorine gas changes from 3.00 L to 1.00 L while maintaining the temperature and the number of moles constant. To solve for the final pressure of the chlorine gas, we can use Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure of the gas is inversely proportional to its volume (P1V1 = P2V2).

Setting up the equation with the known values, we have:
1.60 atm * 3.00 L = P2 * 1.00 L
Solving for P2 (final pressure), we find:
P2 = (1.60 atm * 3.00 L) / 1.00 L
P2 = 4.80 atm

Therefore, the final pressure of chlorine gas, when compressed to a volume of 1.00 L, is 4.80 atm provided that the temperature and the amount of chlorine remain constant.

Answer 2

The final pressure of a gas is calculated using Bolyes law formula

that is P1V1 =P2V2
p1=1.6 atm
V1=3.0L
V2= 1.0L
P2=?

P2 is = P1V1/V2

= 1.6 atm x3.0L /1.0 L = 4.8 atm