The only naturally occurring isotopes of nitrogen are N-14 and N-15. Based on the atomic mass of the element nitrogen on the Periodic Table, compare the relative abundances of the naturally occurring isotopes of nitrogen

Isotope N–14 = 99%

Isotope N–15 = 1%

Explanation:

Let isotope A be N-14

Let isotope B be N-15

From the question given above, the following data were obtained:

For isotope A (N-14):

Mass of A = 14

Abundance of A = A%

For isotope B (N-15):

Mass of B = 15

Abundance of B = (100 – A%)%

Atomic mass of nitrogen = 14.01 amu

Thus, we can obtain the relative abundances of the naturally occurring isotopes of nitrogen as illustrated below:

Atomic mass = [(Mass of A × A%)/100] + [(Mass of B × B%)/100]

14.01 = [(14 × A%)/100] + [(15 × (100 – A%)/100]

14.01 = 0.14A% + 0.15(100 – A%)

14.01 = 0.14A% + 15 – 0.15A%

Collect like terms

14.01 – 15 = 0.14A% – 0.15A%

– 0.99 = – 0.01A%

Divide both side by – 0.01

A% = – 0.99 / –0.01

A% = 99%

Abundance of B = (100 – A%)%

Abundance of B = (100 – 99)%

Abundance of B = 1%

Thus, the relative abundances of the naturally occurring isotopes of nitrogen are:

Isotope N–14 = 99%

Isotope N–15 = 1%

i believe the answer is c. "baking" is the gerund, while "baking blueberry muffins" would be the gerund phrase. hope this ! : )

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.