`H_(2)S` burns in `O_(2)` to form

Options

A. `H_(2)O + S`
B. `H_(2)O + SO_(2)`
C. `H_(2)O + SO_(3)`
D. `H_(2)SO_(4) + S`

Answer

To solve the question, we need to determine the products formed when hydrogen sulfide (H₂S) burns in oxygen (O₂). Here’s a step-by-step solution:

### Step 1: Write the Reactants
The reactants in this reaction are hydrogen sulfide (H₂S) and oxygen (O₂).

### Step 2: Identify the Products
When hydrogen sulfide burns in oxygen, it typically produces water (H₂O) and sulfur dioxide (SO₂).

### Step 3: Write the Chemical Equation
The unbalanced chemical equation for the reaction is:
\[ \text{H}_2\text{S} + \text{O}_2 \rightarrow \text{H}_2\text{O} + \text{SO}_2 \]

### Step 4: Balance the Chemical Equation
To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation.

1. Start with the sulfur (S) atoms. There is 1 S in H₂S and 1 S in SO₂, so sulfur is balanced.
2. Next, balance the hydrogen (H) atoms. There are 2 H in H₂S and 2 H in 2 H₂O, so we need 2 H₂O:
\[ \text{H}_2\text{S} + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} + \text{SO}_2 \]
3. Now, balance the oxygen (O) atoms. On the right side, there are 2 O in 2 H₂O and 2 O in SO₂, totaling 4 O. Therefore, we need 2 O₂ on the left:
\[ 2 \text{H}_2\text{S} + 3 \text{O}_2 \rightarrow 2 \text{H}_2\text{O} + 2 \text{SO}_2 \]

### Step 5: Final Balanced Equation
The final balanced equation is:
\[ 2 \text{H}_2\text{S} + 3 \text{O}_2 \rightarrow 2 \text{H}_2\text{O} + 2 \text{SO}_2 \]

### Conclusion
Thus, when hydrogen sulfide burns in oxygen, it forms water (H₂O) and sulfur dioxide (SO₂). Therefore, the correct answer is:
**Water and Sulfur Dioxide (Option B).**

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