The element boron exists in nature as two isotopes: 10b has a mass of 10.0129 u, and 11b has a mass of 11.0093 u. the average atomic mass of boron is 10.81 u. calculate the relative abundance (as percentages) of the two boron isotopes.

The relative abundance of 10B = 0.20 (20%)

The relative abundance of 11B = 0.80 (80%)

Explanation:

Step 1: Data given

Boron has 2 natural isotopes

⇒ 10B has a mass of 10.0129 u

⇒ 11B has a mass of 11.0093 u

Average atomic mas of Boron = 10.81

Step 2:

10B has an abundance of X %

11B has an abundance of Y %

X+ Y = 1

X = 1 - Y

10.81 = 10.0129* (1 - Y) + 11.0093*Y

10.81 = 10.0129 - 10.0129Y + 11.0093Y

0.7971 = 0.9964Y

Y = 0.80

X = 1.0 - 0.80 = 0.20

10.0129*0.20 + 11.0093*0.80 = 2.00258 +8.8044 = 10.81

The relative abundance of 10B = 0.20 (20%)

The relative abundance of 11B = 0.80 (80%)

false

because it does not have the potential to be entirely used up

it should be all of them because it asks if you included all of those in your answer

explanation: