An arctic weather balloon is filled with 32.3L of helium gas inside a prep shed. The temperature inside the shed is 8.°C. The balloon is then taken outside, where the temperature is 10.°C. Calculate the new volume of the balloon.You may assume the pressure on the balloon stays constant at exactly 1atm. Be sure your answer has the correct number of significant digits.

This problem can be solved using the ideal gas law, which states that the volume of a gas is directly proportional to its temperature, as long as the pressure and the amount of gas remain constant. This relationship is expressed in the formula V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

Here are the steps to solve the problem:

1. Convert the initial and final temperatures from Celsius to Kelvin. The Kelvin scale is the standard unit of temperature in physics, and it starts at absolute zero (0K), which is -273.15°C. So, to convert from Celsius to Kelvin, you add 273.15 to the Celsius temperature.

   T1 = 8.°C + 273.15 = 281.15K T2 = 10.°C + 273.15 = 283.15K

2. Substitute the known values into the formula and solve for V2.

   (32.3L / 281.15K) = V2 / 283.15K V2 = (32.3L / 281.15K) * 283.15K V2 = 32.5L

So, the volume of the balloon outside is approximately 32.5L. This answer has three significant digits, which is appropriate given the number of significant digits in the problem statement.