Question

3. 2.20 L of air at 1.10 atm is allowed to expand to fill a 6.30 L container. Find the final pressure.

Answer 1

Answer:

P₂ = 0.38  atm

Explanation:

Given data:

Volume of air = 2.20 L

Initial pressure = 1.10 atm

Final volume = 6.30 L

Final pressure = ?

Solution:

The given problem will be solved through the Boly's law,

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume  

Now we will put the values in formula,

P₁V₁ = P₂V₂

1.10 atm × 2.20 L = P₂  × 6.30 L

P₂ = 2.42 atm. L/  6.30 L

P₂ = 0.38  atm

Answer 2

Answer:

Final pressure of air would be 0.38 atm

Explanation:

2.20 Liters of air at an atmospheric pressure is allowed to expand to fill a container of 6.30 Liters. We have to find the final pressure of the air.

Assuming that temperature remains constant during this process, we can apply Boyle's Law to this scenario. According to the Boyle's Law:

If the temperature of a gas remains same, the pressure of a gas is inversely proportion to its volume. In mathematical form Boyle's Law can be expressed as:

$P_{1}V_{1}=P_{2}V{2}$

Here, P1 and V1 are initial pressure and volume and P2 and V2 are final ones after the expansion.

Using the given values, we get:

$2.20 \times 1.10 = P_{2} \times 6.30\\\\ P_{2} = 0.38$

Thus, the final pressure of the air, considering a constant temperature, would be 0.38 atm.