An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 125 amu and 127 amu, with natural abundances of 45% and 55%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place

The average atomic mass is 126.1

Explanation:

To obtain the atomic mass of the isotope we use this formula;

(% composition of isotope 1 * mass number) + (% composition of isotope 2 * mass number)

1. Equate the percentage composition with the mass number of each isotope

45/100 * 125 = 56.25

55/100 * 127 = 69.85

2. Add both answers together you get,

56.25 + 69.85 = 126.1.

The average atomic mass is therefore 126.1

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

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