Question

a sample of gas initially occupies 5.50 liter at a pressure of 0.750 atm at 13.0 C. what will the temperture change to 22.5 C and the volume is chnaged to 1.50 L

Answer 1

Answer:

The pressure will be 2.84 atm

Explanation:

The gas laws are a set of chemical and physical laws that allow us to determine the behavior of gases in a closed system. The parameters evaluated in these laws are pressure, volume, temperature and moles.

Boyle's law indicates that the volume is inversely proportional to the pressure: if the pressure increases, the volume decreases and if the pressure decreases, the volume increases. Boyle's law is expressed mathematically as:

P * V = k

On the other hand, Charles's law indicates that with increasing temperature, the volume of the gas increases and with decreasing temperature, the volume of the gas decreases. That is, they are directly proportional. This is expressed mathematically as:

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

Finally, the Gay-Lussac law says that at constant volume, the pressure of the gas is directly proportional to its temperature. Mathematically, it is expressed 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:

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

When you want to study two different states, an initial and a final one of a gas, you can use the following expression:

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

In this case:

• P1= 0.750 atm
• V1= 5.50 L
• T1= 13 C= 286 K (being 0 C=273 K)
• P2=?
• V2= 1.50 L
• T2= 22.5 C=295.5 K

Replacing:

$\frac{0.750 atm*5.50 L}{286 K}= \frac{P2*1.50 L}{295.5 K}$

Solving:

$P2=\frac{295.5K}{1.50L} *\frac{0.750 atm*5.50 L}{286 K}$

P2= 2.84 atm

The pressure will be 2.84 atm