Nitrogen has two isotopes. one has an atomic mass of 14.003
amu and a relative abundance of 99.63% while the other
isotope has an atomic mass of 15.000 amu and a relative
abundance of 0.37%. what is the average atomic mass for
nitrogen?
a
14.456 amu
b
14.778 amu
c 14.993 amu
d 14.007 amu

d= 14.007 amu

Explanation:

Abundance of N¹⁴ = 99.63%

Abundance of N¹⁵ = 0.37%

Atomic mass of N¹⁴ = 14.003 amu

Atomic mass of N¹⁵ = 15.000 amu

Average atomic mass = ?

Solution:

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

Average atomic mass = (14.003 × 99.63)+(15.000× 0.37) /100

Average atomic mass =  1395.12 + 5.55 / 100

Average atomic mass  = 1400.67/ 100

Average atomic mass = 14.007 amu.

away from the curb

explanation:

the wheels would then hit the curb if it started to rolling, decreasing the chance of an accident.

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be