Element X has two natural isotopes:X-6 (6.015amu) and X-7 (7.016amu). calculate the atomic mass of element X given the abundance of X-7 is 92.5%.

a)12.5amu
b)6.50amu
c)6.09amu
d)6.52amu
e)6.94amu

6.940925 amu

Can be rounded off to two decimal places as 6.94 amu

If X-7 is 92.5%, then X-6 must be 100-92.5 = 7.5%

Then 6.015(0.075) + 7.016(0.925) = ??

6.94amu

Element X has two naturally occurring isotopes, X-6 which has a percent abundance of 92.41%, and X-7 which has an unknown abundance. Determine the percent abundance of X-7.

Element A has two isotopes. The first isotope is present 17.7% of the time and has a mass of 248.89. The second isotope has a mass of 206.58. Calculate the atomic mass of element A.

To calculate the atomic mass of element X, we first need to calculate the weighted average of the masses of its isotopes.

Given that the abundance of X-7 is 92.5%, we can deduce that the abundance of X-6 is 100% - 92.5% = 7.5%.

Next, we calculate the weighted average using the formula:

Atomic mass = (abundance of isotope 1 * mass of isotope 1) + (abundance of isotope 2 * mass of isotope 2)

Atomic mass = (0.925 * 7.016 amu) + (0.075 * 6.015 amu)

Atomic mass = 6.48 + 0.451

Atomic mass ≈ 6.931 amu

Therefore, the atomic mass of element X is approximately 6.931 amu.

Based on the answer choices provided, the closest option is e) 6.94 amu.

6.4 aum