A person skied from the top of a mountain to the base of the mountain with a balloon tied to each of her ski p

Question

Top (elevation = 9970 feet, TO = -10 oC, P623 mm Hg)

Bottom (elevation = 6920 feet, T = -5 oC, P = 688 mm Hg)

Answer 1

(p1t1)/V1=(p2T2).v2

Answer 2

PV=nRT

nR=PV/T

(P1*V1)/T1=(P2*V2)/T2

°K  = °C+273.15

multiply each side by T2

T2*(P1*V1)/T1=(P2*V2)

Divide both sides by P2

T2*(P1*V1)/(T1*P2)=V2

(263.15°K  * 623 mm Hg * 2 L)/ (268.15°K  * 688 mm Hg) ≈ 1.78 L

Answer 3

You would use the Ideal Gas Law to figure this out.

PV = nRT

where

P = pressure

V = volume

n = the number of moles of gas

R = the universal gas constant (which you can look up if you don't already know what this is)

T = temperature

(1) PV = nRT (using the values for the top of the mountain:  P, V, R, T)

(2) solve for n

(3) PV = nRT (using the values for the bottom of the mountain: P, n, R, T)

(4) solve for V.