A 1.0 L rubber balloon is filled with carbon dioxide gas is an warm (25.0°C) room (pressure = 745 mm Hg). What volume will the gas occupy when it is taken out into the open air where the temperature is -12° C and the pressure is 742 mm Hg?

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

10 years is the answer

the answer is symmetrical : )