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

Answer:

The volume will be 12.05 L

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:

$\frac{V}{T} =k$

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:

$\frac{P}{T}=k$

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

$\frac{P*V}{T}=k$

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

$\frac{P1*V1}{T1}=\frac{P2*V2}{T2}$

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:

$\frac{0.956 atm*14.3L}{296 K}=\frac{1.20 atm*V2}{313 K}$

Solving for V2:

$V2= \frac{313 K}{1.20 atm} *\frac{0.956 atm*14.3L}{296 K}$

V2= 12.05 L

The volume will be 12.05 L