What mass of H2SO4 must be employed in the reaction `BaCl_(2)+H_(2)SO_(4)rarr BaSO_(4)+2HCl` if `2 2.08gBaCl_(2)` is used up and `2.33gBaSO4 , 0.73gHCl` are formed.

Options

A. 0.98 g
B. 1.23 g
C. 0.72 g
D. 0.49g

Answer

To determine the mass of H₂SO₄ required in the reaction \( \text{BaCl}_2 + \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{HCl} \), given that 22.08 g of BaCl₂ is used and 2.33 g of BaSO₄ and 0.73 g of HCl are formed, we can follow these steps:

### Step 1: Calculate the number of moles of BaSO₄ produced.

To find the number of moles of BaSO₄, we use the formula:
\[ \text{Number of moles} = \frac{\text{Given mass}}{\text{Molar mass}} \]
The molar mass of BaSO₄ (Barium Sulfate) is approximately:
- Ba: 137.33 g/mol
- S: 32.07 g/mol
- O: 16.00 g/mol × 4 = 64.00 g/mol

Calculating the molar mass:
\[ \text{Molar mass of BaSO}_4 = 137.33 + 32.07 + 64.00 = 233.40 \text{ g/mol} \]

Now, we can calculate the number of moles of BaSO₄ produced:
\[ \text{Number of moles of BaSO}_4 = \frac{2.33 \text{ g}}{233.40 \text{ g/mol}} \approx 0.00998 \text{ moles} \]

### Step 2: Determine the number of moles of H₂SO₄ required.

From the balanced chemical equation, we see that 1 mole of H₂SO₄ produces 1 mole of BaSO₄. Thus, the moles of H₂SO₄ required will be equal to the moles of BaSO₄ produced:
\[ \text{Number of moles of H}_2\text{SO}_4 = 0.00998 \text{ moles} \]

### Step 3: Calculate the mass of H₂SO₄ needed.

To find the mass of H₂SO₄, we again use the formula:
\[ \text{Mass} = \text{Number of moles} \times \text{Molar mass} \]
The molar mass of H₂SO₄ is:
- H: 1.01 g/mol × 2 = 2.02 g/mol
- S: 32.07 g/mol
- O: 16.00 g/mol × 4 = 64.00 g/mol

Calculating the molar mass:
\[ \text{Molar mass of H}_2\text{SO}_4 = 2.02 + 32.07 + 64.00 = 98.09 \text{ g/mol} \]

Now we can calculate the mass of H₂SO₄:
\[ \text{Mass of H}_2\text{SO}_4 = 0.00998 \text{ moles} \times 98.09 \text{ g/mol} \approx 0.978 \text{ g} \]

### Final Answer:
The mass of H₂SO₄ that must be employed in the reaction is approximately **0.98 g**.

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