The average mass of a nitrogen atom is 14.006 amu from the two isotopes with the following data: 14N-14.00307 amu with 0.9963 fractional abundance; 1SN- 15.000108 amu with 0.00364 fractional abundance. Calculate the percentage abundance of each isotopic form. Select the correct answer below: a. 13.95% and 0.05%, respectively b. 0.054% and 0.638%, respectively c. 9.63% and 0.0364%, respectively d. 99.63% and 0.364%, respectively

d. 99.63% and 0.364%, respectively

Explanation:

The average mass of a nitrogen atom is 14.006 amu

14N-14.00307 amu with 0.9963 fractional abundance

1SN- 15.000108 amu with 0.00364 fractional abundance.

The relative abundance definition in chemistry is the percentage of a particular isotope that occurs in nature. The atomic mass listed for an element on the periodic table is an average mass of all known isotopes of that element.

In this problem, the fractional abundance has areaady been given. All we need to do now is convert them to percentage abundance.

14N-14.00307 = 0.9963* 100% = 99.63%

1SN- 15.000108 = 0.00364 * 100% = 0.364%

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.