IDNLearn.com provides a seamless experience for finding accurate answers. Ask anything and receive prompt, well-informed answers from our community of experienced experts.
Sagot :
To determine the theoretical yield of [tex]\( Fe_2(SO_4)_3 \)[/tex] from the given reaction, we will follow these steps:
### Step 1: Understand the Balanced Equation
The balanced chemical reaction is as follows:
[tex]\[ 2 \ FePO_4 + 3 \ Na_2SO_4 \rightarrow Fe_2(SO_4)_3 + 2 \ Na_3PO_4 \][/tex]
### Step 2: Identify Molar Masses
From the information provided:
- Molar mass of [tex]\( FePO_4 \)[/tex] = 150.82 g/mol
- Molar mass of [tex]\( Fe_2(SO_4)_3 \)[/tex] = 399.88 g/mol
### Step 3: Calculate Moles of [tex]\( FePO_4 \)[/tex]
Given mass of [tex]\( FePO_4 \)[/tex] = 20.00 g
Number of moles of [tex]\( FePO_4 \)[/tex] is calculated using the formula:
[tex]\[ \text{moles of } FePO_4 = \frac{\text{mass of } FePO_4}{\text{molar mass of } FePO_4} \][/tex]
[tex]\[ \text{moles of } FePO_4 = \frac{20.00 \ \text{g}}{150.82 \ \text{g/mol}} \approx 0.1326 \ \text{mol} \][/tex]
### Step 4: Use Stoichiometry to Find Moles of [tex]\( Fe_2(SO_4)_3 \)[/tex]
From the balanced equation:
[tex]\[ 2 \ \text{moles of } FePO_4 \rightarrow 1 \ \text{mole of } Fe_2(SO_4)_3 \][/tex]
Therefore, the moles of [tex]\( Fe_2(SO_4)_3 \)[/tex] produced:
[tex]\[ \text{moles of } Fe_2(SO_4)_3 = \frac{0.1326 \ \text{mol} \ FePO_4}{2} = 0.0663 \ \text{mol} \][/tex]
### Step 5: Calculate the Theoretical Yield (Mass) of [tex]\( Fe_2(SO_4)_3 \)[/tex]
The mass of [tex]\( Fe_2(SO_4)_3 \)[/tex] is:
[tex]\[ \text{mass of } Fe_2(SO_4)_3 = \text{moles of } Fe_2(SO_4)_3 \times \text{molar mass of } Fe_2(SO_4)_3 \][/tex]
[tex]\[ \text{mass of } Fe_2(SO_4)_3 = 0.0663 \ \text{mol} \times 399.88 \ \text{g/mol} \approx 26.52 \ \text{g} \][/tex]
### Final Answer
The theoretical yield of [tex]\( Fe_2(SO_4)_3 \)[/tex] when 20.00 g of [tex]\( FePO_4 \)[/tex] reacts with an excess of [tex]\( Na_2SO_4 \)[/tex] is approximately 26.52 g.
### Step 1: Understand the Balanced Equation
The balanced chemical reaction is as follows:
[tex]\[ 2 \ FePO_4 + 3 \ Na_2SO_4 \rightarrow Fe_2(SO_4)_3 + 2 \ Na_3PO_4 \][/tex]
### Step 2: Identify Molar Masses
From the information provided:
- Molar mass of [tex]\( FePO_4 \)[/tex] = 150.82 g/mol
- Molar mass of [tex]\( Fe_2(SO_4)_3 \)[/tex] = 399.88 g/mol
### Step 3: Calculate Moles of [tex]\( FePO_4 \)[/tex]
Given mass of [tex]\( FePO_4 \)[/tex] = 20.00 g
Number of moles of [tex]\( FePO_4 \)[/tex] is calculated using the formula:
[tex]\[ \text{moles of } FePO_4 = \frac{\text{mass of } FePO_4}{\text{molar mass of } FePO_4} \][/tex]
[tex]\[ \text{moles of } FePO_4 = \frac{20.00 \ \text{g}}{150.82 \ \text{g/mol}} \approx 0.1326 \ \text{mol} \][/tex]
### Step 4: Use Stoichiometry to Find Moles of [tex]\( Fe_2(SO_4)_3 \)[/tex]
From the balanced equation:
[tex]\[ 2 \ \text{moles of } FePO_4 \rightarrow 1 \ \text{mole of } Fe_2(SO_4)_3 \][/tex]
Therefore, the moles of [tex]\( Fe_2(SO_4)_3 \)[/tex] produced:
[tex]\[ \text{moles of } Fe_2(SO_4)_3 = \frac{0.1326 \ \text{mol} \ FePO_4}{2} = 0.0663 \ \text{mol} \][/tex]
### Step 5: Calculate the Theoretical Yield (Mass) of [tex]\( Fe_2(SO_4)_3 \)[/tex]
The mass of [tex]\( Fe_2(SO_4)_3 \)[/tex] is:
[tex]\[ \text{mass of } Fe_2(SO_4)_3 = \text{moles of } Fe_2(SO_4)_3 \times \text{molar mass of } Fe_2(SO_4)_3 \][/tex]
[tex]\[ \text{mass of } Fe_2(SO_4)_3 = 0.0663 \ \text{mol} \times 399.88 \ \text{g/mol} \approx 26.52 \ \text{g} \][/tex]
### Final Answer
The theoretical yield of [tex]\( Fe_2(SO_4)_3 \)[/tex] when 20.00 g of [tex]\( FePO_4 \)[/tex] reacts with an excess of [tex]\( Na_2SO_4 \)[/tex] is approximately 26.52 g.
We value your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. Discover insightful answers at IDNLearn.com. We appreciate your visit and look forward to assisting you again.