# How do you calculate the average atomic mass of rubidium if 72.17% of its atoms have a mass of 84.91 amu and 27.83% of its atoms have a mass of 86.91 amu?

The average atomic mass of some substance is measured indeed with the percentages of how much they exist in nature. An average is always calculated by adding up the numbers and divide that by the amount of number you had, so, for example, the average for the numbers 1, 3, and two times 7 is:

If we now look at the percentage of the numbers encountered we see that we encounter 25% the number 1 25% the number 3 50% the number 7

From the total of all rubidium, you will encounter 72.17% times the 84.91 amu one, and 27.83% times the 86.91 amu one. We use exactly the same approach as in the example above:

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To calculate the average atomic mass of rubidium, multiply the mass of each isotope by its respective abundance percentage, then add the products together. For rubidium: Average atomic mass = (0.7217 * 84.91 amu) + (0.2783 * 86.91 amu)

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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