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Answer :
Let's solve this problem step-by-step:
1. Understand the Problem: We need to find how many moles of chlorine atoms are present in a certain number of molecules of dinitrogen trichloride, [tex]\(N_2Cl_3\)[/tex].
2. Given Data:
- Number of [tex]\(N_2Cl_3\)[/tex] molecules: [tex]\(1.64 \times 10^{23}\)[/tex]
- Avogadro's Number, which is the number of molecules in one mole of a substance: [tex]\(6.022 \times 10^{23}\)[/tex]
3. Calculate Moles of Dinitrogen Trichloride (N\_2Cl\_3):
- To determine the moles of [tex]\(N_2Cl_3\)[/tex], divide the number of molecules by Avogadro's number:
[tex]\[
\text{Moles of } N_2Cl_3 = \frac{1.64 \times 10^{23}}{6.022 \times 10^{23}} \approx 0.272 \text{ moles}
\][/tex]
4. Calculate Moles of Chlorine Atoms:
- Each molecule of [tex]\(N_2Cl_3\)[/tex] contains 3 chlorine atoms.
- Therefore, to find the number of moles of chlorine atoms, multiply the moles of [tex]\(N_2Cl_3\)[/tex] by 3:
[tex]\[
\text{Moles of chlorine atoms} = 0.272 \times 3 \approx 0.817 \text{ moles}
\][/tex]
5. Conclusion: Therefore, there are approximately 0.817 moles of chlorine atoms in [tex]\(1.64 \times 10^{23}\)[/tex] molecules of dinitrogen trichloride.
The correct answer is 0.817 mol.
1. Understand the Problem: We need to find how many moles of chlorine atoms are present in a certain number of molecules of dinitrogen trichloride, [tex]\(N_2Cl_3\)[/tex].
2. Given Data:
- Number of [tex]\(N_2Cl_3\)[/tex] molecules: [tex]\(1.64 \times 10^{23}\)[/tex]
- Avogadro's Number, which is the number of molecules in one mole of a substance: [tex]\(6.022 \times 10^{23}\)[/tex]
3. Calculate Moles of Dinitrogen Trichloride (N\_2Cl\_3):
- To determine the moles of [tex]\(N_2Cl_3\)[/tex], divide the number of molecules by Avogadro's number:
[tex]\[
\text{Moles of } N_2Cl_3 = \frac{1.64 \times 10^{23}}{6.022 \times 10^{23}} \approx 0.272 \text{ moles}
\][/tex]
4. Calculate Moles of Chlorine Atoms:
- Each molecule of [tex]\(N_2Cl_3\)[/tex] contains 3 chlorine atoms.
- Therefore, to find the number of moles of chlorine atoms, multiply the moles of [tex]\(N_2Cl_3\)[/tex] by 3:
[tex]\[
\text{Moles of chlorine atoms} = 0.272 \times 3 \approx 0.817 \text{ moles}
\][/tex]
5. Conclusion: Therefore, there are approximately 0.817 moles of chlorine atoms in [tex]\(1.64 \times 10^{23}\)[/tex] molecules of dinitrogen trichloride.
The correct answer is 0.817 mol.
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