A 5 mole sample of liquid acetone is converted to a gas at 75.0 degrees Celsius. If 628.00 J is required to raise the temperature of the liquid to its boiling point, 15.60 kJ is required to evaporate the liquid, and 712.00 J is required to raise the final temperature to 75.0 degrees Celsius, what is the total energy required for the conversion

16.94 kJ  

Explanation:

Energy to reach boiling point =       628.00 J

    Energy to evaporate liquid = 15 600  

           Energy to heat vapour =       712.00

                                     TOTAL = 16 940       J

                                                 = 16.94 kJ

The total energy required is 16.94 kJ.

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.