Looking for answers? Westonci.ca is your go-to Q&A platform, offering quick, trustworthy responses from a community of experts. Discover comprehensive solutions to your questions from a wide network of experts on our user-friendly platform. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.
Sagot :
To determine the number of molecules in a 23.45 g sample of copper(II) hydroxide, [tex]\( Cu(OH)_2 \)[/tex], we need to follow these steps:
1. Convert the mass of the sample to moles:
The molar mass of copper(II) hydroxide ([tex]\( Cu(OH)_2 \)[/tex]) is given as [tex]\( 97.562 \, \text{g/mol} \)[/tex]. This means that 1 mole of [tex]\( Cu(OH)_2 \)[/tex] weighs [tex]\( 97.562 \, \text{g} \)[/tex].
First, calculate the number of moles in a [tex]\( 23.45 \, \text{g} \)[/tex] sample using the relationship:
[tex]\[ \text{Number of moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \][/tex]
So,
[tex]\[ \text{Number of moles} = \frac{23.45 \, \text{g}}{97.562 \, \text{g/mol}} \approx 0.2404 \, \text{mol} \][/tex]
2. Convert moles to molecules:
One mole of any substance contains Avogadro's number of molecules, which is [tex]\( 6.022 \times 10^{23} \)[/tex] molecules per mole.
To find the number of molecules in the given number of moles, use the relationship:
[tex]\[ \text{Number of molecules} = \text{Number of moles} \times \text{Avogadro's number} \][/tex]
Thus,
[tex]\[ \text{Number of molecules} = 0.2404 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} \][/tex]
[tex]\[ \text{Number of molecules} \approx 1.447 \times 10^{23} \, \text{molecules} \][/tex]
In conclusion, a 23.45 g sample of [tex]\( Cu(OH)_2 \)[/tex] contains approximately [tex]\( 0.2404 \, \text{moles} \)[/tex] and [tex]\( 1.447 \times 10^{23} \)[/tex] molecules of [tex]\( Cu(OH)_2 \)[/tex]. These results are expressed to the correct number of significant figures based on the given values in the problem.
1. Convert the mass of the sample to moles:
The molar mass of copper(II) hydroxide ([tex]\( Cu(OH)_2 \)[/tex]) is given as [tex]\( 97.562 \, \text{g/mol} \)[/tex]. This means that 1 mole of [tex]\( Cu(OH)_2 \)[/tex] weighs [tex]\( 97.562 \, \text{g} \)[/tex].
First, calculate the number of moles in a [tex]\( 23.45 \, \text{g} \)[/tex] sample using the relationship:
[tex]\[ \text{Number of moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}} \][/tex]
So,
[tex]\[ \text{Number of moles} = \frac{23.45 \, \text{g}}{97.562 \, \text{g/mol}} \approx 0.2404 \, \text{mol} \][/tex]
2. Convert moles to molecules:
One mole of any substance contains Avogadro's number of molecules, which is [tex]\( 6.022 \times 10^{23} \)[/tex] molecules per mole.
To find the number of molecules in the given number of moles, use the relationship:
[tex]\[ \text{Number of molecules} = \text{Number of moles} \times \text{Avogadro's number} \][/tex]
Thus,
[tex]\[ \text{Number of molecules} = 0.2404 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} \][/tex]
[tex]\[ \text{Number of molecules} \approx 1.447 \times 10^{23} \, \text{molecules} \][/tex]
In conclusion, a 23.45 g sample of [tex]\( Cu(OH)_2 \)[/tex] contains approximately [tex]\( 0.2404 \, \text{moles} \)[/tex] and [tex]\( 1.447 \times 10^{23} \)[/tex] molecules of [tex]\( Cu(OH)_2 \)[/tex]. These results are expressed to the correct number of significant figures based on the given values in the problem.
We hope our answers were useful. Return anytime for more information and answers to any other questions you have. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Thank you for using Westonci.ca. Come back for more in-depth answers to all your queries.