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 1.85 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

Answer:

P₂ = 5.55 atm

Explanation:

Mathematically, Boyle's law can be stated as:

${\displaystyle P\propto {\frac {1}{V}}}$

Pressure is inversely proportional to the volume

${\displaystyle PV=k}$ Pressure multiplied by volume equals some constant ${\displaystyle k}$

where P is the pressure of the gas, V is the volume of the gas, and k is a constant.

The equation states that the product of pressure and volume is a constant for a given mass of confined gas and this holds as long as the temperature is constant. For comparing the same substance under two different sets of conditions, the law can be usefully expressed as:

${\displaystyle P_{1}V_{1}=P_{2}V_{2}$

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

that is  P1V1 =P2V2

Because the temperature and number of moles remained constant, we can use the formula

P₁V₁=P₂V₂

3.00 L * 1.85 atm = P₂ * 1.00 L

P₂ = 5.55 atm

Answer 2

Answer:

Explanation:

since the problem involves pressure and volume, boyle's law is used.

P1V1= P2V2

P1 = 1.85 atm

P2 =?????

V1