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Update:A balloon is filled with He gas to a volume of 2.10 L at 35 °C. The balloon is placed in liquid nitrogen until its temperature reaches –196 °C. Assuming the pressure remains constant, what is the volume of the cooled balloon?
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Verified answer
Use Charles' Law since pressure is constant: V1/T1 = V2/T2
Find the temperature in kelvins first.
T1= 35°C +273.15= 308 K
T2= -196°C + 273.15 = 77 K
V1=2.10 L
V2= x
Plug into the equation
2.10 L/ 308 K = x / 77 K
cross multiply
160 L*K = 308 K *x
divide 308 K over
x=0.52 L
The cooled balloon has a volume of 0.52 Liters,
This is a Charles' law application: V₁/T₁ = V₂/T₂. Remember that temperatures must be expressed in Kelvins - K = °C + 273. 35°C = 308 K; -196°C = 77-K. Charles' law states that the volume of a confined gas is directly proportional to its Kelvin temperature.
2.10-L / 308-K = V₂/77-K ===> V₂ = 0.525-L
In this problem, the temperature decreases from 308-K to 77-K - a four-fold decrease (308/77=4). This means that the volume should also experience a four-fold decrease. 2.10/4 = 0.525