Question

A sealed balloon is filled with 2.20 liters of helium gas at 20.0°

c. if the pressure does not change, what is the temperature when the balloon expands to a volume of 2.60 liters

Answer 1

The temperature when the balloon expands to 2.60 L is 346 K

Step-by-step explanation:

Given:

Initial volume of the ballon, V1 = 2.20 L

Initial Temperature, T1 = 20 C

Final volume of the ballon, V2 = 2.60 L

To determine:

Final Temperature, T2

Step-by-step explanation:

Based on the ideal gas equation

`PV = nRT`

where P = pressure, V = volume ; n = moles of gas

R = gas constant, T = temperature

At constant n and P, the above equation becomes:

V/T = constant

This is the Charles law

Therefore:

`(V1)/(T1) = (V2)/(T2) \\\\T2 = (V2)/(V1)*T1 = (2.60L)/(2.20L)*(20+273)K = 346 K`

Answer 2

To solve this we assume that the gas inside the balloon is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant pressure and number of moles of the gas the ratio T/V is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

T1 / V1 = T2 / V2

T2 = T1 x V2 / V1

T2 = 20 x 2.60 / 2.20

T2 = 23.64 degrees Celsius