The volume of air in a balloon is 4.5 liters when inflated. External pressure decreases the volume to 1.1 liters. If the original pressure was 1.00 atmosphere, what pressure would be required to produce that change if everything else is constant?
4.1 atm right?
4.5Lx1.00atm=1.1LxPf
equation looks good ... Boyle's Law
constant temp
P1V1=P2V2
P2=P1*V1/V2=1atm*4.5/1.1= 4atm
To find the pressure required to produce the change in volume, you can use the formula:
(Volume1 x Pressure1) = (Volume2 x Pressure2)
Given:
Volume1 = 4.5 liters
Pressure1 = 1.00 atmosphere
Volume2 = 1.1 liters
Using the formula, we can rearrange it to solve for Pressure2:
Pressure2 = (Volume1 x Pressure1) / Volume2
Substituting the values:
Pressure2 = (4.5 L x 1.00 atm) / 1.1 L
Pressure2 = 4.09 atm
Therefore, the pressure required to produce the change in volume is approximately 4.09 atmospheres.
To find the pressure required to produce the change in volume, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
Boyle's Law equation is: P₁V₁ = P₂V₂
Given:
V₁ = 4.5 liters (initial volume)
V₂ = 1.1 liters (final volume)
P₁ = 1.00 atmosphere (initial pressure)
We can substitute the given values into the equation and solve for P₂:
P₁V₁ = P₂V₂
1.00 atm * 4.5 L = P₂ * 1.1 L
4.5 atm = 1.1 P₂
Now, divide both sides of the equation by 1.1 to isolate P₂:
4.5 atm / 1.1 = P₂
Calculating the result:
P₂ ≈ 4.09 atm
Therefore, the pressure required to produce the change in volume from 4.5 liters to 1.1 liters, under the given conditions, is approximately 4.09 atmospheres.