Question

g An arctic weather balloon is filled with 31.0 L of helium gas inside a prep shed. The temperature inside the shed is 7. C. The balloon is then taken outside, where the temperature is -35. C. Calculate the new volume of the balloon. You may assume the pressure on the balloon stays constant at exactly 1 atm. Be sure your answer has the correct number of significant digits.

Answer 1

The new volume at at temperature of -35 °C is 26.4 L

Step-by-step explanation:

Step 1: Data given

Volume of the helium gas inside a prep shed = 31.0 L

The temperature inside the shed is 7.0 °C = 7+273 = 280 K

The balloon is then taken outside, where the temperature is -35. C = 273 -35 = 238K

The pressure on the balloon stays constant at exactly 1 atm

Step 2: Calculate the new volume

V1/T1 = V2/T2o

⇒with V1 = the original volume of the helium gas inside a prep shed = 31.0 L

⇒with T1 = the original temperature inside the shed = 280 K

⇒with V2 = the new volume of the helium gas inside a prep shed = TO BE DETERMINED

⇒with T2 = the decreased temperature = 238 K

31.0 L / 280 K = V2 / 238 K

V2 = (31.0L / 280K) * 238 K

V2 = 26.35 ≈ 26.4 L

The new volume at at temperature of -35 °C is 26.4 L

Answer 2

Final volume of ballon is 26.4L

Step-by-step explanation:

It is possible to answer this question using Charles's law that is the law that describes how a gas expands when temperature increases at constant pressure. The formula is:

`(V_1)/(T_1) =(V_2)/(T_2)`

Where V is volume in liters, T is absolute temperature (In kelvin) and 1 represents initial state while 2 represents final states.

Initial volume: 31.0L

Initial temperature: 273.15 + 7 = 280.15K

Final temperature: 273.15 - 35 = 238.15K

`(31.0L)/(280.15K) =(V_2)/(238.15K)`

V₂ = 26.4L

That means final volume of ballon is 26.4L