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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 17 options: 15.0 L 30.0 L 60.0 L 120.0 L

Respuesta :

MathPhys

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

Answer:

60.0L

Step-by-step explanation:

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