Answer to Question #110894 in Chemistry for Faisy

Question

If the temperature of the helium balloon were increased from 30°C to 35°C and the volume of the balloon only expanded from 0.47L to 1.55L, how much pressure would be inside the balloon?

Answer 1

According to the gas law equation:

p₁V₁/T₁ = p₂V₂/T₂

where p₁ - initial pressure, V₁ - initial volume, T₁ - initial temperature, p₂ - final pressure, V₂ - final volume, T₂ - final temperature.

From here:

p₁/p₂ = V₂T₁/V₁T₂

As 30°C = 303.15 K and 35°C = 308.15 K:

p₁/p₂ = 1.55 L × 303.15 K / 0.47 L × 308.15 K = 3.24

As a result, the pressure in the ballon is 3.24 times lower compared to the initial pressure.