A balloon contains 7.2 L of He. Th
e pressure is reduced to 2.00 atm and the
balloon expands to occupy a volume of
25.1 L. What was the initial pressure
exerted on the balloon?
I got 0.57 ml, but the answer says 7.0 ml.
I am not sure if my answer is wrong of correct?
P1 V1 = P2 V2
7.1 P1 = 50.2
P1 = 7.07 atm
I do not know why it says mL when you are using liters L Anyway the answer is in ATMOSPHERES pressure, not milliliters or Liters
To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
We can set up the equation using Boyle's Law as follows:
(P1)(V1) = (P2)(V2)
Where:
P1 = initial pressure (unknown)
V1 = initial volume (7.2 L)
P2 = final pressure (2.00 atm)
V2 = final volume (25.1 L)
Plugging in the given values, we can solve for P1:
(P1)(7.2 L) = (2.00 atm)(25.1 L)
To solve for P1, divide both sides of the equation by 7.2 L:
P1 = (2.00 atm)(25.1 L) / (7.2 L)
Calculating this gives us:
P1 = 6.97 atm
So, the initial pressure exerted on the balloon was approximately 6.97 atm.
It seems that there might have been an error in your calculations. Please check your calculations again to see if you made a mistake along the way.
To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
The equation for Boyle's Law is:
P1 x V1 = P2 x V2
Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume
Given:
V1 = 7.2 L
P2 = 2.00 atm
V2 = 25.1 L
We need to find P1, the initial pressure.
Using the equation for Boyle's Law, we can rearrange it to solve for P1:
P1 = (P2 x V2) / V1
Substituting the given values:
P1 = (2.00 atm x 25.1 L) / 7.2 L
P1 = 50.2 atm * L / 7.2 L
P1 ≈ 6.972 atm
Therefore, the initial pressure exerted on the balloon was approximately 6.972 atm, not 0.57 ml or 7.0 ml.
It seems like there might be an error in the answer provided. The correct answer should be approximately 6.972 atm.