Answer: (17684.85x) / 221712 L.
Explanation: To determine the volume of the gas-filled weather balloon at the higher altitude, we can use the combined gas law equation:
P1V1 / T1 = P2V2 / T2
Where:
P1 = initial pressure (at ground level) = unknown
V1 = initial volume (at ground level) = 60.5 L
T1 = initial temperature (at ground level) = 25°C = 298 K
P2 = final pressure (at higher altitude) = 744 mmHg
V2 = final volume (at higher altitude) = unknown
T2 = final temperature (at higher altitude) = 20°C = 293 K
We need to solve for V2, the final volume.
Let's rearrange the equation to solve for V2:
V2 = (P1V1T2) / (P2T1)
To find P1, we need to convert the initial pressure from mmHg to atm (atmospheres). 1 atm is approximately equal to 760 mmHg.
Let's assume P1 = x atm.
Substituting the values into the equation:
V2 = (x * 60.5 * 293) / (744 * 298)
Simplifying the equation:
V2 = (17684.85x) / 221712
Therefore, the volume of the gas-filled weather balloon at the higher altitude is (17684.85x) / 221712 L.
Note: We need the value of P1 (initial pressure) to calculate the final volume accurately. Without this information, we cannot determine the exact volume at the higher altitude.