A helium-filled balloon has a volume of 50.0 L at 25°C and 1.08 atm. What volume will it have at .855 atm and 10.0°C? Question 1
7 options: 15.0 L 30.0 L 60.0 L 120.0 L
1 answer:
Answer:
60.0 L
Step-by-step explanation:
Ideal gas law:
PV = nRT
where P is absolute pressure,
V is volume,
n is number of moles,
R is gas constant,
and T is absolute temperature.
Since n and R don't change:
P₁V₁ / T₁ = P₂V₂ / T₂
(1.08 atm) (50.0 L) / (25 + 273.15 K) = (0.855 atm) V / (10 + 273.15 K)
V = 60.0 L
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