We appreciate your visit to Naturally occurring strontium consists of four isotopes Sr 84 Sr 86 Sr 87 and Sr 88 Below is the data concerning strontium Sr 84 83. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!
Answer :
Final answer:
To determine the mass and percent abundance of Strontium-88, we can use the information provided. By subtracting the percent abundances of the other isotopes from 100%, we can find the percent abundance of Sr-88. Using the formula for average atomic mass, we can solve for the mass of Sr-88.
Explanation:
To determine the mass and percent abundance of Strontium-88, we can use the information provided. Given that Sr-84 has a mass of 83.913 amu and a percent abundance of 0.56%, Sr-86 has a mass of 85.909 amu and a percent abundance of 9.86%, and Sr-87 has a mass of 86.909 amu and a percent abundance of 7.00%, we can calculate the mass and percent abundance of Sr-88.
Considering that the total percent abundances of all four strontium isotopes must add up to 100%, we can find the percent abundance of Sr-88 by subtracting the percent abundances of Sr-84, Sr-86, and Sr-87 from 100%: 100% - 0.56% - 9.86% - 7.00% = 82.58%.
Since the average atomic mass of strontium is provided, we can use the formula for average atomic mass to calculate the mass of Sr-88: Average atomic mass = (% abundance x mass) + (% abundance x mass) + (% abundance x mass) + (% abundance x mass).
Plugging in the values for all the isotopes: (0.56% x 83.913 amu) + (9.86% x 85.909 amu) + (7.00% x 86.909 amu) + (82.58% x mass of Sr-88) = average atomic mass of strontium.
Solving for the mass of Sr-88:
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