Calculate average atomic mass: 25% c-11, 25% c-14

6.25 amu

Explanation:

Data Given:

Abundance of C-11 = 25 % = 0.25

mass of carbon-11 = 11 amu

Abundance of C-14 = 25 % = 0.25

mass of carbon-14 = 14 amu

Average atomic mass = ?

Solution:

formula used to check average atomic mass is as under

                          Average atomic mass = m₁A₁ + m₂A₂

Where

m₁ and m₂ = mass of isotope 1 and 2 respectively

A₁ and A₂ = abundance or fraction of isotope 1 and 2 respectively

Put values in above formula

                   Average atomic mass = (11 amu)(0.25) + (14 amu)(0.25)    

                   Average atomic mass = 2.75 + 3.5

                   Average atomic mass = 6.25 amu

So

Average atomic mass of 25% C-11, 25% C-14 = 6.25 amu

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

explanation: no but i do not usually comment