To solve this problem, we need to set up an equation based on the definition of average atomic mass. The average atomic mass is the sum of the masses of its isotopes, each multiplied by its natural abundance.

Let's denote the percent abundance of isotope A as p. Since the percent abundance of isotope B is the rest of the 100%, it can be represented as (100% - p).

The equation can be set up as follows:

63.092 = 64.531p/100 + 62.126(100 - p)/100

To solve for p, we first multiply through by 100 to get rid of the denominator:

6309.2 = 64.531p + 6212.6 - 62.126p

Then, we combine like terms:

2.405p = 96.6

Finally, we divide both sides by 2.405 to solve for p:

p = 96.6 / 2.405 ≈ 40.12%

So, the percent abundance of isotope A is approximately 40.12%.

Question

To solve this problem, we need to set up an equation based on the definition of average atomic mass. The average atomic mass is the sum of the masses of its isotopes, each multiplied by its natural abundance.

Let's denote the percent abundance of isotope A as p. Since the percent abundance of isotope B is the rest of the 100%, it can be represented as (100% - p).

The equation can be set up as follows:

63.092 = 64.531p/100 + 62.126(100 - p)/100

To solve for p, we first multiply through by 100 to get rid of the denominator:

6309.2 = 64.531p + 6212.6 - 62.126p

Then, we combine like terms:

2.405p = 96.6

Finally, we divide both sides by 2.405 to solve for p:

p = 96.6 / 2.405 ≈ 40.12%

So, the percent abundance of isotope A is approximately 40.12%.

Knowee AI · Accepted Answer

To solve this problem, we need to set up an equation based on the definition of average atomic mass. The average atomic mass is the sum of the masses of its isotopes, each multiplied by its natural abundance.

Let's denote the percent abundance of isotope A as p. Since the percent abundance of isotope B is the rest of the 100%, it can be represented as (100% - p).

The equation can be set up as follows:

63.092 = 64.531p/100 + 62.126(100 - p)/100

To solve for p, we first multiply through by 100 to get rid of the denominator:

6309.2 = 64.531p + 6212.6 - 62.126p

Then, we combine like terms:

2.405p = 96.6

Finally, we divide both sides by 2.405 to solve for p:

p = 96.6 / 2.405 ≈ 40.12%

So, the percent abundance of isotope A is approximately 40.12%.

A hypothetical element X has two naturally occurring isotopes: A with an isotopic mass of 64.531 and B with an isotopic mass of 62.126. If the element X has an atomic mass of 63.092, what is the percent abundance of isotope A?

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