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Chapter 2: Problem 4

What is the mass (in amu) of a) \(100^{12} \mathrm{C}\) atoms? b) \(100^{13} \mathrm{C}\) atoms?

Short Answer

Expert verified
a) The mass of \(100^{12}\mathrm{C}\) atoms is 1200 amu. b) The mass of \(100^{13}\mathrm{C}\) atoms is 1300 amu.

Step by step solution

01

Identify the average atomic mass

The average atomic mass of every isotope is given by the number on the top of the element symbol. Thus, the average atomic mass of \(^{12}C\) is 12 amu and the average atomic mass of \(^{13}C\) is 13 amu.
02

Calculate the total mass for \(^{12}C\) atoms

Multiply the total number of atoms, in this case, 100 with the average atomic mass of \(^{12}C\) (which is 12 amu) to get the total mass. Therefore, total mass = 100 * 12 amu = 1200 amu.
03

Calculate the total mass for \(^{13}C\) atoms

Similar to Step 2, the total mass of \(^{13}C\) can be calculated by multiplying the total number of atoms, in this case, 100 with the average atomic mass of \(^{13}C\) (which is 13 amu). Therefore, total mass = 100 * 13 amu = 1300 amu.

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Most popular questions from this chapter

How many isotopes of magnesium occur naturally on Earth?

Give two interpretations of the number "12.011" found below the symbol for carbon on the periodic table.

Which has more atoms: \(1.008 \mathrm{~g}\) of hydrogen or \(39.95 \mathrm{~g}\) of argon? Explain your reasoning.

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