Question

A balloon was partially filled with helium gas at room temperature. It occupied 4.0 liters of volume at 700.0 mmHg atmospheric pressure. When the balloon was released, it traveled upward until it burst at 99 mmHg atmospheric pressure. (Neglect any force exerted to stretch the rubber balloon.) What was the volume of the balloon when it burst? L

Answer 1

28.28 L.

Step-by-step explanation:

• We can use the general law of ideal gas: PV = nRT.

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

• If n and T are constant, and have two different values of V and P:

P₁V₁ = P₂V₂

P₁ = 700.0 mm Hg, V₁ = 4.0 L.

at burst: P₂ = 99.0 mm Hg, V₂ = ??? L.

∴ V₂ = P₁V₁/P₂ = (700.0 mm Hg)(4.0 L)/(99.0 mm Hg) = 28.28 L.