How many moles of lead (II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g of HCl?

Options

A. `0.333`
B. `0.011`
C. `0.029`
D. `0.044`

Explanation

To determine how many moles of lead (II) chloride (PbCl2) will be formed from the reaction between 6.5 g of lead(II) oxide (PbO) and 3.2 g of hydrochloric acid (HCl), we will follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between lead(II) oxide and hydrochloric acid can be represented as follows:

\[ \text{PbO} + 2 \text{HCl} \rightarrow \text{PbCl}_2 + \text{H}_2\text{O} \]

### Step 2: Calculate the molar mass of PbO
- Lead (Pb) has a molar mass of approximately 207.2 g/mol.
- Oxygen (O) has a molar mass of approximately 16.0 g/mol.

Thus, the molar mass of PbO is:

\[ \text{Molar mass of PbO} = 207.2 + 16.0 = 223.2 \, \text{g/mol} \]

### Step 3: Calculate the number of moles of PbO
Using the formula for moles:

\[ \text{Number of moles} = \frac{\text{Given mass}}{\text{Molar mass}} \]

For PbO:

\[ \text{Number of moles of PbO} = \frac{6.5 \, \text{g}}{223.2 \, \text{g/mol}} \approx 0.0291 \, \text{moles} \]

### Step 4: Calculate the molar mass of HCl
- Hydrogen (H) has a molar mass of approximately 1.0 g/mol.
- Chlorine (Cl) has a molar mass of approximately 35.5 g/mol.

Thus, the molar mass of HCl is:

\[ \text{Molar mass of HCl} = 1.0 + 35.5 = 36.5 \, \text{g/mol} \]

### Step 5: Calculate the number of moles of HCl
Using the same formula for moles:

For HCl:

\[ \text{Number of moles of HCl} = \frac{3.2 \, \text{g}}{36.5 \, \text{g/mol}} \approx 0.0877 \, \text{moles} \]

### Step 6: Determine the limiting reactant
From the balanced equation, 1 mole of PbO reacts with 2 moles of HCl. Therefore, for 0.0291 moles of PbO, the required moles of HCl would be:

\[ \text{Required moles of HCl} = 2 \times 0.0291 = 0.0582 \, \text{moles} \]

Since we have 0.0877 moles of HCl available, HCl is in excess, and PbO is the limiting reactant.

### Step 7: Calculate the number of moles of PbCl2 formed
According to the balanced equation, 1 mole of PbO produces 1 mole of PbCl2. Therefore, the number of moles of PbCl2 formed will be equal to the number of moles of PbO:

\[ \text{Number of moles of PbCl2} = 0.0291 \, \text{moles} \]

### Final Answer
The number of moles of lead (II) chloride (PbCl2) formed from the reaction is approximately **0.0291 moles**.

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