White phosphorus reacts with chlorine and the product hydrolyses in the presence of water. Calcualte the mass of HCl obtained by the hydrolysis of the product formed by the reaction of 62 g of white phosphorus with chlorine in the presence of water.

Options

A. 200 g
B. 400 g
C. 219 g
D. 100 g

Explanation

To solve the problem, we need to follow these steps:

### Step 1: Write the balanced chemical equations
First, we need to write the balanced equations for the reaction of white phosphorus (P4) with chlorine (Cl2) and the subsequent hydrolysis.

1. The reaction of white phosphorus with chlorine:
\[ P_4 + 6Cl_2 \rightarrow 4PCl_3 \]

2. The hydrolysis of phosphorus trichloride (PCl3):
\[ 4PCl_3 + 12H_2O \rightarrow 4H_3PO_3 + 12HCl \]

### Step 2: Calculate the number of moles of P4
Next, we need to calculate the number of moles of P4 in 62 grams.

- Molar mass of P4 = 4 × 31 = 124 g/mol
- Number of moles of P4:
\[ \text{Number of moles} = \frac{\text{Given mass}}{\text{Molar mass}} = \frac{62 \, \text{g}}{124 \, \text{g/mol}} = 0.5 \, \text{moles} \]

### Step 3: Use stoichiometry to find moles of HCl produced
From the balanced equations, we see that 1 mole of P4 produces 12 moles of HCl. Therefore, 0.5 moles of P4 will produce:
\[ \text{Moles of HCl} = 0.5 \, \text{moles P4} \times 12 \, \text{moles HCl/mole P4} = 6 \, \text{moles HCl} \]

### Step 4: Calculate the mass of HCl produced
Now, we need to calculate the mass of HCl produced using the number of moles calculated.

- Molar mass of HCl = 1 + 35.5 = 36.5 g/mol
- Mass of HCl:
\[ \text{Mass of HCl} = \text{Number of moles} \times \text{Molar mass} = 6 \, \text{moles} \times 36.5 \, \text{g/mol} = 219 \, \text{g} \]

### Final Answer
The mass of HCl obtained by the hydrolysis of the product formed by the reaction of 62 g of white phosphorus with chlorine in the presence of water is **219 grams**.

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