For the following elements, calculate the average atomic mass. Carbon-12 98.93%, Carbon-13 1.07% *

Average atomic mass of carbon = 12.01 amu

Explanation:

Given data:

Average atomic mass = ?

Percent abundance of C-12 = 98.93%

Percent abundance of C-13 = 1.07%

Solution:

Average atomic mass of carbon = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass)  / 100

Average atomic mass of carbon = (98.93×12)+(1.07×13) /100

Average atomic mass of carbon=  1187.16 + 13.91 / 100

Average atomic mass of carbon = 1201.07/ 100

Average atomic mass of carbon = 12.01 amu

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.