A weather balloon at Earth's surface has a volume of 4.00 L at 304 K and 755 mm Hg.?

If the balloon is released and the volume reaches 4.08 L at 728 mm Hg, what is the temperature? What gas law do you use?

(P1V1)/T1 = P2V2)/T2

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To solve this problem, you can use the combined gas law, which states that:

(P₁ * V₁) / T₁ = (P₂ * V₂) / T₂

Where:
P₁ and P₂ are the initial and final pressures, respectively.
V₁ and V₂ are the initial and final volumes, respectively.
T₁ and T₂ are the initial and final temperatures, respectively.

In this case, the initial conditions are:
P₁ = 755 mm Hg
V₁ = 4.00 L
T₁ = 304 K

The final conditions are:
P₂ = 728 mm Hg
V₂ = 4.08 L

Now, let's plug in the values to solve for T₂:

(755 mm Hg * 4.00 L) / 304 K = (728 mm Hg * 4.08 L) / T₂

303920 / 304 K = 296704 / T₂

T₂ = (296704 * 304 K) / 303920

T₂ ≈ 296.81 K

Therefore, the temperature T₂ is approximately 296.81 K.

The gas law used in this problem is the combined gas law.

To solve this problem, we can use the combined gas law. The combined gas law equation is given as:

(P1 * V1) / (T1) = (P2 * V2) / (T2)

In this equation:
P1 and P2 represent the initial and final pressures respectively,
V1 and V2 represent the initial and final volumes respectively,
T1 and T2 represent the initial and final temperatures respectively.

In the given problem, we know:
P1 = 755 mm Hg
V1 = 4.00 L
T1 = 304 K
V2 = 4.08 L
P2 = 728 mm Hg

To find T2, we can rearrange the equation and solve for T2:

T2 = (P2 * V2 * T1) / (P1 * V1)

Substituting the values into the equation:

T2 = (728 mm Hg * 4.08 L * 304 K) / (755 mm Hg * 4.00 L)

Calculating this expression:

T2 ≈ 288 K

Therefore, the temperature T2 is approximately 288 K.

The gas law used in this problem is the combined gas law, which relates the pressure, volume, and temperature of a gas when the other variables are changed while keeping the amount of gas constant. This law is applicable when a gas is kept in a closed system and the conditions change.