Question

answer asap please

A sealed balloon is filled with air at atmospheric pressure (P = 1.01 X 105 Pa) at 30°C (typical conditions for the surface of the Earth in St. Thomas). You take the (sealed) balloon with you on top of Mountain Top, which has an elevation of about 450m, where the average air pressure is 9.6 x 109 Pa. The temperature at the top is 26°C, a bit cooler. 2.5 pts. - a) How big is the balloon on top of the mountain (top) compared to its size at sea level (V...)? Express your answer as the ratio Vto/sea 2 pts. - b) The average human breath takes in about 500 cm of air. Calculate the number of moles of air in a breath at sea level on St. Thomas at 30°C. 3 pts. - c) Calculate the number of moles of air in a breath at Mountain Top on St. Thomas at 26°C.

Answer 1

From gas laws

$\frac{P_{1}V_{1}}{T_{1}}=\frac{P_{2}V_{2}}{T_{2}}$

$\frac{P_{1}T_{2}}{P_{2}T_{1}}=\frac{V_{2}}{V_{1}}$

$\frac{V_{2}}{V_{1}}=1.038$

b)

we know PV=nRT

R = 0.082057 L-atm /mol K

putting P= 1 atm and T= 303 K

we get

n= 0.0201 moles

c)

now P = 0.95 atm

T =299 K

we get n= 0.0193

d)

We from from kinetic theory of gases

K.E= 3/2nRT

where K.E is kinetic energy

so K.E = 1.5 X 8.314 X 303

= 3778.713 J/mol

e)

for process under constant volume

molar heat capacity = Cv

given the gas is diatomic so Cv =5/2 R

now Q= nCv$\Delta T$

Q=7690.45 J