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amid [387]
3 years ago
7

A helium-filled weather balloon has a volume of 512 L at 18.9°C and 756 mmHg. It is released and rises to an altitude of 2.14 km

, where the pressure is 639 mmHg and the temperature is 5.9°C.
The volume of the balloon at this altitude is
L.
Chemistry
2 answers:
Ad libitum [116K]3 years ago
8 0

Answer:

578.8 L

Explanation:

In order to solve this problem, we can use the equation of state for an ideal gas, which states that:

pV=nRT

where

p is the pressure of the gas

V is its volume

n is the number of moles

R is the gas constant

T is the absolute temperature of the gas

The equation can also be rewritten as

\frac{pV}{T}=nR

For a gas transformation, the term on the right (nR) is constant, so we can write:

\frac{p_1 V_1}{T_1}=\frac{p_2 V_2}{T_2}

where in this problem:

p_1 = 756 mm Hg is the initial pressure of the gas

V_1=512 L is the initial volume

T_1=18.9^{\circ}+273=291.9 K is the initial temperature

p_2 = 639 mm Hg is the final pressure

T_2=5.9^{\circ}C+273=278.9 K is the final temperature

Solving for V2, we find the final volume of the balloon:

V_2=\frac{p_1 V_1T_2}{T_1p_2}=\frac{(756)(512)(278.9)}{(291.9)(639)}=578.8 L

vazorg [7]3 years ago
3 0

633.97 L

Explanation:

Well use the combined gas law;

P₁V₁T₁ = P₂V₂T₂

We need to change the temperatures into Kelvin;

18.9°C= 292.05 K

5.9°C = 279.05 K

756 * 512 * 292.05 = 639 * V₂ * 279.05

113,044,377.6 = 178,312.95 V₂

V₂ = 113,044,377.6 / 178,312.95

V₂ = 633.97 L

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