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

Final pressure will be 0.308 times the initial pressure

Step-by-step explanation:

To solve this problem, we can use the equation of state for an ideal gas:

`pV=nRT`

where

p is the gas pressure

V is the volume of the gas

n is the number of moles

R is the gas constant

T is the absolute temperature of the gas

For a gas under transformation, we can write the equation as:

`(p_1 V_1)/(T_1)=(p_2 V_2)/(T_2)`

where for the gas in this problem:

`p_1` = is the initial pressure (not given)

`V_1=0.47 L` is the initial volume

`T_1=30C+273=303 K` is the initial temperature

`p_2 =` is the final pressure

`V_2=1.55 L` is the final volume

`T_2=35+273 = 308 K` is the final temperature

Solving for p2, we find:

`p_2 = (p_1 V_1 T_2)/(T_1 V_2)=(p_1 (0.47)(308))/((303)(1.55))=0.308p_1`