Answer :
Sure! Let's find out how many [tex]\( \text{Ca}^{2+} \)[/tex] ions are present in 6.00 moles of [tex]\( \text{CaO} \)[/tex].
1. Understand the Problem:
- We have 6.00 moles of calcium oxide ([tex]\( \text{CaO} \)[/tex]).
- We want to determine the number of [tex]\( \text{Ca}^{2+} \)[/tex] ions in it.
2. Key Concept:
- Calcium oxide ([tex]\( \text{CaO} \)[/tex]) is composed of calcium ions ([tex]\( \text{Ca}^{2+} \)[/tex]) and oxide ions ([tex]\( \text{O}^{2-} \)[/tex]). In one mole of calcium oxide, there is one mole of calcium ions.
3. Avogadro's Number:
- Avogadro's number is [tex]\( 6.022 \times 10^{23} \)[/tex], which tells us how many particles (atoms, molecules, ions) are in one mole of a substance.
4. Calculate the Number of [tex]\( \text{Ca}^{2+} \)[/tex] Ions:
- Since 1 mole of [tex]\( \text{CaO} \)[/tex] contains 1 mole of [tex]\( \text{Ca}^{2+} \)[/tex] ions, the number of ions in 6.00 moles of [tex]\( \text{CaO} \)[/tex] is equal to 6.00 moles of [tex]\( \text{Ca}^{2+} \)[/tex] ions.
5. Multiplication:
- Multiply the number of moles of [tex]\( \text{CaO} \)[/tex] by Avogadro's number to get the number of [tex]\( \text{Ca}^{2+} \)[/tex] ions:
[tex]\[
6.00 \, \text{moles} \times 6.022 \times 10^{23} \, \text{ions/mole} = 3.6132 \times 10^{24} \, \text{ions}
\][/tex]
So, there are [tex]\( 3.6132 \times 10^{24} \)[/tex] [tex]\( \text{Ca}^{2+} \)[/tex] ions in 6.00 moles of [tex]\( \text{CaO} \)[/tex].
1. Understand the Problem:
- We have 6.00 moles of calcium oxide ([tex]\( \text{CaO} \)[/tex]).
- We want to determine the number of [tex]\( \text{Ca}^{2+} \)[/tex] ions in it.
2. Key Concept:
- Calcium oxide ([tex]\( \text{CaO} \)[/tex]) is composed of calcium ions ([tex]\( \text{Ca}^{2+} \)[/tex]) and oxide ions ([tex]\( \text{O}^{2-} \)[/tex]). In one mole of calcium oxide, there is one mole of calcium ions.
3. Avogadro's Number:
- Avogadro's number is [tex]\( 6.022 \times 10^{23} \)[/tex], which tells us how many particles (atoms, molecules, ions) are in one mole of a substance.
4. Calculate the Number of [tex]\( \text{Ca}^{2+} \)[/tex] Ions:
- Since 1 mole of [tex]\( \text{CaO} \)[/tex] contains 1 mole of [tex]\( \text{Ca}^{2+} \)[/tex] ions, the number of ions in 6.00 moles of [tex]\( \text{CaO} \)[/tex] is equal to 6.00 moles of [tex]\( \text{Ca}^{2+} \)[/tex] ions.
5. Multiplication:
- Multiply the number of moles of [tex]\( \text{CaO} \)[/tex] by Avogadro's number to get the number of [tex]\( \text{Ca}^{2+} \)[/tex] ions:
[tex]\[
6.00 \, \text{moles} \times 6.022 \times 10^{23} \, \text{ions/mole} = 3.6132 \times 10^{24} \, \text{ions}
\][/tex]
So, there are [tex]\( 3.6132 \times 10^{24} \)[/tex] [tex]\( \text{Ca}^{2+} \)[/tex] ions in 6.00 moles of [tex]\( \text{CaO} \)[/tex].
