Questions: Part B How many moles of aluminum ions are present in 0.36 moles of Al2(SO4)3? Express the number of moles to two significant figures. nAl= square mol Submit Request Answer Part C How many moles of sulfate ions (SO4 2-) are present in 1.7 moles of Al2(SO4)3? Express the number of moles to two significant figures. square Submit Request Answer

Part B

How many moles of aluminum ions are present in 0.36 moles of Al2(SO4)3?
Express the number of moles to two significant figures.
nAl= square mol
Submit
Request Answer

Part C

How many moles of sulfate ions (SO4 2-) are present in 1.7 moles of Al2(SO4)3?
Express the number of moles to two significant figures.
square
Submit
Request Answer

Transcript text: Part B How many moles of aluminum ions are present in 0.36 moles of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ ? Express the number of moles to two significant figures. \[ n_{\mathrm{Al}}=\square \mathrm{mol} \] Submit Request Answer Part C How many moles of sulfate ions $\left(\mathrm{SO}_{4}{ }^{2-}\right)$ are present in 1.7 moles of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ ? Express the number of moles to two significant figures. $\square$ Submit Request Answer

Solution

Solution Steps

Step 1: Determine the number of aluminum ions in one formula unit of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$

Each formula unit of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ contains 2 aluminum ions ($\mathrm{Al}^{3+}$).

Step 2: Calculate the total moles of aluminum ions

Given 0.36 moles of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$, we multiply by the number of aluminum ions per formula unit: \[ 0.36 \, \text{moles of} \, \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} \times 2 \, \text{moles of} \, \mathrm{Al}^{3+} \, \text{per mole of} \, \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} = 0.72 \, \text{moles of} \, \mathrm{Al}^{3+} \]

Final Answer for Part B

\[ \boxed{n_{\mathrm{Al}} = 0.72 \, \text{mol}} \]

Step 1: Determine the number of sulfate ions in one formula unit of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$

Each formula unit of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ contains 3 sulfate ions ($\mathrm{SO}_{4}^{2-}$).

Step 2: Calculate the total moles of sulfate ions

Given 1.7 moles of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$, we multiply by the number of sulfate ions per formula unit: \[ 1.7 \, \text{moles of} \, \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} \times 3 \, \text{moles of} \, \mathrm{SO}_{4}^{2-} \, \text{per mole of} \, \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} = 5.1 \, \text{moles of} \, \mathrm{SO}_{4}^{2-} \]

Final Answer for Part C

\[ \boxed{5.1 \, \text{mol}} \]

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