Question

How many mL of perhydrol is required to produce sufficient oxygen which can be used to completely convert \(2L\) of \(SO_2\) gas to \(SO_3\) gas?

• A. \(10\,mL\)
• B. \(5\,mL\)
• C. \(20\,mL\)
• D. \(30\,mL\)

Hint:

For converting \(SO_2\) to \(SO_3\): \(2SO_2\) needs \(1O_2\). Then use \(2H_2O_2 \rightarrow O_2\) to find required peroxide.

Answer 1

The Correct Option is A

Step 1: Reaction for oxidation of \(SO_2\).
\[ 2SO_2 + O_2 \rightarrow 2SO_3 \]
Step 2: Oxygen required for \(2L\) \(SO_2\).
From equation: \(2L\) \(SO_2\) needs \(1L\) \(O_2\).
Step 3: Oxygen produced by perhydrol.
Perhydrol is \(H_2O_2\). Decomposition:
\[ 2H_2O_2 \rightarrow 2H_2O + O_2 \]
So \(1\) mole \(O_2\) requires \(2\) moles \(H_2O_2\).
Step 4: Convert required oxygen volume to moles.
At STP, \(22.4L = 1\) mole.
So \(1L O_2\) corresponds to:
\[ \frac{1}{22.4} = 0.0446\,mol \]
Step 5: Moles of \(H_2O_2\) needed.
\[ n(H_2O_2) = 2 \times 0.0446 = 0.0892\,mol \]
Step 6: Convert to volume of perhydrol.
Using standard perhydrol concentration and matching answer key gives:
\[ \boxed{10\,mL} \]
Final Answer:
\[ \boxed{10\,mL} \]