Question

A balloon that had a volume of 3.50 L at 25.0°C is placed in a hot room at 40.0°C. If the pressure remains constant at 1.00 atm, what is the new volume of the balloon in the hot room? Use mc005-1.jpg.

Answer 1

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

V2 = T2 x V1 / T1

V2 = 313.15 x 3.50 / 298.15

V2 = 3.68 L

Answer 2

What is the final volume of the balloon after it has been placed in the hot room?      

3.68  wrong

⇒ 2.1 L  the correct on E.D.G.