Boron has an average atomic mass of 10.81. one isotope of boron has a mass of 10.012938 and a relative abundance of 19.80 percent . the other isotope has a relative abundance of 80.20 percent what is the mass of that isotope? report two decimal places

The atomic mass of the second isotope of boron (B) is 11.01 amu.

Explanation:

The average atomic mass is can be calculated by the summation of the product of the atomic mass of each isotope multiplied by its abundance (abundance % / 100.0).Boron has two isotopes:

1) At.mass = 10.012938 amu ≅ 10.013 amu and its abundance = 0.198

2) At.mass = ??? amu and its abundance = 0.802

Average atomic mass of boron = 10.81 amu.

The average atomic mass of boron = (10.013 amu)*(0.198) + (atomic mass of the second isotope amu)*(0.802) = 10.81 amu10.81 = 1.9825 + (0.802 x atomic mass of the second isotope)(0.802 x atomic mass of the second isotope) = 10.81 - 1.9825 = 8.8275.Atomic mass of the second isotope = 8.8275 / 0.802 = 11.0068 ≅ 11.01 amu.

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.

2.00 is the !