Answer :
To find the molar mass of the unknown compound, follow these steps:
1. Understand the given information:
- We have a sample with a mass of 1.00 grams.
- The number of molecules in this sample is 8.35 x 10²¹.
2. Recall Avogadro's number:
- Avogadro's number is 6.022 x 10²³ molecules per mole. This is a constant that helps us convert between the number of molecules and moles.
3. Calculate the number of moles in the sample:
- To determine how many moles are represented by 8.35 x 10²¹ molecules, we use the formula:
[tex]\[
\text{moles} = \frac{\text{number of molecules}}{\text{Avogadro's number}}
\][/tex]
- Plug in the given values:
[tex]\[
\text{moles} = \frac{8.35 \times 10^{21}}{6.022 \times 10^{23}}
\][/tex]
4. Calculate the molar mass:
- Molar mass is defined as the mass of one mole of a substance. The formula is:
[tex]\[
\text{molar mass} = \frac{\text{mass of the sample}}{\text{number of moles}}
\][/tex]
- Substitute the values:
[tex]\[
\text{molar mass} = \frac{1.00 \text{ g}}{0.013865825307206908 \text{ mol}}
\][/tex]
5. Determine the answer:
- The calculated molar mass is 72.12 g/mol.
Therefore, the molar mass of the unknown molecular compound is closest to 72.1 g/mol. So, the correct answer is:
72.1 g/mol
1. Understand the given information:
- We have a sample with a mass of 1.00 grams.
- The number of molecules in this sample is 8.35 x 10²¹.
2. Recall Avogadro's number:
- Avogadro's number is 6.022 x 10²³ molecules per mole. This is a constant that helps us convert between the number of molecules and moles.
3. Calculate the number of moles in the sample:
- To determine how many moles are represented by 8.35 x 10²¹ molecules, we use the formula:
[tex]\[
\text{moles} = \frac{\text{number of molecules}}{\text{Avogadro's number}}
\][/tex]
- Plug in the given values:
[tex]\[
\text{moles} = \frac{8.35 \times 10^{21}}{6.022 \times 10^{23}}
\][/tex]
4. Calculate the molar mass:
- Molar mass is defined as the mass of one mole of a substance. The formula is:
[tex]\[
\text{molar mass} = \frac{\text{mass of the sample}}{\text{number of moles}}
\][/tex]
- Substitute the values:
[tex]\[
\text{molar mass} = \frac{1.00 \text{ g}}{0.013865825307206908 \text{ mol}}
\][/tex]
5. Determine the answer:
- The calculated molar mass is 72.12 g/mol.
Therefore, the molar mass of the unknown molecular compound is closest to 72.1 g/mol. So, the correct answer is:
72.1 g/mol
