A scuba diver takes a 2.8 L balloon from the surface where the pressure is 1.00 atm and the temperature is 34.0 °C to a depth of 25 m, where the pressure is 3.5 atm and the temperature is 18.0 °C. What is the volume of the balloon at this depth?

See your long list of posts for one that changes P, V, and T from one set to another. Same formula.

efref

To find the volume of the balloon at the given depth, we can use Boyle's Law, which states that the volume of a given amount of gas is inversely proportional to its pressure, assuming the temperature remains constant.

Boyle's Law can be expressed as:

P1 * V1 = P2 * V2

Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume

In this case, the initial pressure is 1.00 atm, the initial volume is 2.8 L, the final pressure is 3.5 atm, and we need to solve for the final volume.

Rearranging the equation, we get:

V2 = (P1 * V1) / P2

Substituting the values into the equation:

V2 = (1.00 atm * 2.8 L) / 3.5 atm

V2 = 0.8 L

Therefore, the volume of the balloon at a depth of 25 m is 0.8 L.