A .60 L sample of nitrogen is heated from 27℃ to 77℃ at a constant pressure. What is the final volume of the gas? (show work please)

CHARLES' LAW

given:

= 600 mL = 0.6 L

= 27 °C = 300.15 L

= 77 °C = 350.15 L

conversion:

= 600 mL (1 L / 1000 mL)

= 0.6 L

= 27 °C + 273.15 K

= 300.15 K

= 77 °C + 273.15 K

= 350.15 K

solution:

= ( × ) ÷

= (0.6 L × 350.15 K) ÷ 300.15 K

= 0.7 L

first one is the correct answer

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.