Question

a sample of helium gas occupies 14.3 L at 23 degrees C and 0.956 atm. What volume will it occupy at 40 degrees C and 1.20 atm

Answer 1

The volume will be 12.05 L

Step-by-step explanation:

Boyle's law says that "The volume occupied by a certain gaseous mass at constant temperature is inversely proportional to pressure" and is expressed mathematically as:

P * V = k

Charles's law states that the volume of a gas is directly proportional to the temperature of the gas. That is, Charles's law is a law that says that when the amount of gas and pressure are kept constant, the ratio between the volume and the temperature will always have the same value:

`(V)/(T) =k`

Finally, Gay-Lussac's law states that at constant volume, the pressure of the gas is directly proportional to its temperature. This is expressed mathematically as:

`(P)/(T)=k`

Combined law equation is the combination of three gas laws called Boyle's, Charlie's and Gay-Lusac's law:

`(P*V)/(T)=k`

Analyzing an initial state 1 and a final state 2, this law can be expressed as:

`(P1*V1)/(T1)=(P2*V2)/(T2)`

In this case:

• P1= 0.956 atm
• V1= 14.3 L
• T1= 23 °C= 296 °K
• P2= 1.20 atm
• V2= ?
• T2= 40 °C= 313 °K

Replacing:

`(0.956 atm*14.3L)/(296 K)=(1.20 atm*V2)/(313 K)`

Solving for V2:

`V2= (313 K)/(1.20 atm) *(0.956 atm*14.3L)/(296 K)`

V2= 12.05 L

The volume will be 12.05 L