Calculate the mass, in grams, of a single rubidium atom ( mRb
  = 85.468  amu
  ).
Express your answer in grams to four significant figures.

To calculate the mass of a single rubidium atom in grams, we can use the following relationship between atomic mass units (amu) and grams:

\[
1 \ \text{amu} = 1.66053906660 \times 10^{-24} \ \text{g}
\]

Given that the mass of a rubidium atom is \( 85.468 \ \text{amu} \), the mass in grams is:

\[
\text{Mass of one rubidium atom} = 85.468 \ \text{amu} \times 1.66053906660 \times 10^{-24} \ \text{g/amu}
\]

Let’s calculate this value.The mass of a single rubidium atom is approximately \( 1.4192 \times 10^{-22} \) grams, expressed to four significant figures.

Would you like further details or have any questions?

Here are five related questions to explore:
1. How do you convert from grams to moles for rubidium?
2. What is the molar mass of rubidium, and how is it related to atomic mass?
3. How do you calculate the number of rubidium atoms in a given mass?
4. What is the significance of atomic mass in chemical reactions?
5. How is the mass of isotopes of an element like rubidium determined?

**Tip:** When converting between atomic mass units and grams, always remember the conversion factor \( 1 \, \text{amu} = 1.66053906660 \times 10^{-24} \, \text{g} \).

Calculate the mass, in grams, of a single rubidium atom (mRb = 85.468 amu). Express your answer in grams to four significant figures.

Learn how to calculate the mass of a single rubidium atom in grams, using the atomic mass (85.468 amu) and the conversion factor between amu and grams. This problem involves key scientific concepts such as atomic mass and unit conversions, suitable for high school students in Grades 9-12.

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