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Calculate the mass in grams of each elemental sample.(a) 1.32 × 1020uranium atoms(b)
Chapter 6, Problem 38P(choose chapter or problem)
Calculate the mass in grams of each elemental sample.
(a) \(1.32 \times 10^{20}\) uranium atoms
(b) \(2.55 \times 10^{22}\) zinc atoms
(c) \(4.11 \times 10^{23}\) lead atoms
(d) \(6.59 \times 10^{24}\) silicon atoms
Equation Transcription:
Text Transcription:
1.32 times 10^20
2.55 times 10^22
4.11 times 10^23
6.59 times 10^24
Questions & Answers
QUESTION:
Calculate the mass in grams of each elemental sample.
(a) \(1.32 \times 10^{20}\) uranium atoms
(b) \(2.55 \times 10^{22}\) zinc atoms
(c) \(4.11 \times 10^{23}\) lead atoms
(d) \(6.59 \times 10^{24}\) silicon atoms
Equation Transcription:
Text Transcription:
1.32 times 10^20
2.55 times 10^22
4.11 times 10^23
6.59 times 10^24
ANSWER:
Solution 38P
Here, we are going to calculate the mass in grams of each of the given elemental sample.
Step 1:
One mole of any species is that quantity in number having a mass equal to its atomic or molecular mass in grams.
The number of particles (atoms, molecules or ions) present in 1 mole of any substance is fixed, with a value of 6.022 × 1023. This is an experimentally obtained value. This number is called the Avogadro Constant or Avogadro Number.