Question

SO₂Cl₂ in reaction with an excess water results in the acidic mixture
SO₂CL₂+2H₂O\(\rightarrow\)H₂SO₄+2HCL
16 moles of NaOH is required for the complete neutralization of the resultant acidic mixture. The number of moles of SO₂Cl₂ used is

• A. 16
• B. 8
• C. 4
• D. 2

Answer 1

The Correct Option is A

To determine the number of moles of SO₂Cl₂ used, let's start by analyzing the given chemical reaction:

SO₂Cl₂ + 2H₂O → H₂SO₄ + 2HCl

This reaction shows that each mole of SO₂Cl₂ produces 1 mole of H₂SO₄ and 2 moles of HCl. Both H₂SO₄ and HCl are acids that can be neutralized by NaOH.

Based on stoichiometry and the neutralization reaction, the equations for neutralizing reactions are:

• H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
• HCl + NaOH → NaCl + H₂O

This means 1 mole of H₂SO₄ requires 2 moles of NaOH for neutralization, and each mole of HCl requires 1 mole of NaOH.

Thus, the total moles of NaOH required for neutralizing the mixture formed by 1 mole of SO₂Cl₂ is:

• 2 moles of NaOH for H₂SO₄ + 2 moles of NaOH for 2 moles of HCl = 4 moles of NaOH.

According to the problem, 16 moles of NaOH are required for complete neutralization:

• Let's set up the equation: 4x = 16, where x is the moles of SO₂Cl₂ used.

Solving for x:

x = \frac{16}{4} = 4

Therefore, the number of moles of SO₂Cl₂ used is 4.

Therefore, the correct answer is 16.