Answer to Question #110907 in Chemistry for Juan Pablo

Question

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

Answer 1

According to the combined 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:

p₂/p₁ = V₁T₂/V₂T₁

As 30°C = 303 K and 35°C = 308 K:

p₂/p₁ = 0.47 L × 308 K / 1.55 L × 303 K = 0.31

As the value is below zero, the final pressure is lower than the initial pressure. After conversion:

p₁/p₂ = 1 / 0.31 = 3.2

Answer: The pressure in the ballon is 3.2 times lower than to the initial pressure.