A balloon filled with helium gas at 20°C occupies 3.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,raising the pressure to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?
A)0.20 L
B)2.6 L
C)5.3 L
D)77 L

Question

Quizplus · Accepted Answer

To solve this problem, we can use the combined gas law, which states that:
(P₁V₁)/T₁ = (P₂V₂)/T₂

Where P₁, V₁, and T₁ are the initial pressure, volume, and temperature of the gas (in Kelvin), respectively, and P₂, V₂, and T₂ are the final pressure, volume, and temperature, respectively.

We can first convert the initial temperature to Kelvin:
T₁ = 20°C + 273.15 = 293.15 K

We can then use the combined gas law to solve for V₂:
(P₁V₁)/T₁ = (P₂V₂)/T₂ 
V₂ = (P₁V₁*T₂)/(P₂*T₁)

Plugging in the values we have:
V₂ = (1.00 atm * 3.91 L * 77 K)/(5.20 atm * 293.15 K)
V₂ = 0.20 L

Therefore, the answer is A) 0.20 L.

A Balloon Filled with Helium Gas at 20°C Occupies 3