A balloon with a pressure of 1 atm and a temperature of 17° Celsius has a volume of 1000 mL. The day warms up and increases the temperature to 27° Celsius, which makes the pressure change to 1520 mm Hg.What is the new volume of the balloon, in Liters?
The new volume of the balloon is <u>0.517 L.</u>
By ideal gas law, PV = nRT
P = pressure
V = volume
n = number of mole of gas
R = gas constant
T = temperature
Using ideal gas law, P₁V₁/ T₁ = P₂V₂/ T₂
P₁= 1 atm
V₁ = 1000 mL = 1 L
T₁ = 17° C = 290 K
After the day warms up:-
P₂ = 1520 mm Hg = 2 atm
T₂ = 27° C = 300 K
Put these values in formula, P₁V₁/ T₁ = P₂V₂/ T₂
V₂ = P₁V₁T₂/ T₁ P₂
V₂ = 1 atm× 1 L × 300 K/ 290 K × 2 atm
V₂ = 0.517 L = 517 mL
Hence, the new volume of the balloon is 0.517 L.
The ideal gas equation is formulated as: PV = nRT.
In this equation, P refers to the pressure of the ideal gas, V is the volume of the ideal gas, n is the overall quantity of ideal gas this is measured in terms of moles, R is the universal gas constant, and T is the temperature.
Learn more about ideal gas law here:- brainly.com/question/25290815
#SPJ1
