Question

A 5.0L balloon in a freezer is at a temperature of - 50 degrees * C has a pressure of 800 mm Hg. What will be the new pressure if the balloon is taken out and placed in a warm room (Temperature 37°C) and the volume expands to 7.0 L?

Answer 1

794 mmHg

Step-by-step explanation:

We are going to be using the Combined Gas Law for this problem as well. Just to refresh out memory - the Combined Gas Law expresses the relationship between pressure, volume, and temperature (in KELVIN) of a fixed amount of gas. The equation itself? Right here:
`(P_(1)V_(1))/(T_(1)) = (P_(2)V_(2))/(T_(2))`

Now, looking at the problem, let's assign the values to its corresponding variable:

P1 = 800mmHg; V1 = 5.0L; T1 = -50°C + 273 = 223K

V2 = 7.0L; T2 = 37°C + 273 = 310K; P2 = ?

We are looking to find the new pressure, a.k.a. P2. So, let's plug and chug the values into the equation.

Set up:
`((800 mmHg)(5.0L))/(223K) = ((7.0L)(P_(2)))/(310K)`

==>
`((800 mmHg)(5.0L))/(223K) * 310K = (7.0L)(P_(2))}`

==>
`P_(2) = ((800 mmHg)(5.0L))/(223K) * (310K)/(7.0) }`

==>
`P_(2) =` 794.36 = 794 mmHg