`H_(4)underline(S_(2))O_(6)+H_(2)O to H_(2)SO_(3)+H_(2)SO_(4)`

Options

A. If product is oxy acid with -ic suffix.
B. If product is oxy acid with -ous suffix
C. If product are two oxy acids one with -ic suffix and otherone with -ous suffix.
D. If product is not oxy acid, neither with -ic suffix nor with -ous suffix

Answer

To solve the question regarding the reaction of \( H_4S_2O_6 + H_2O \) yielding \( H_2SO_3 + H_2SO_4 \), we will follow these steps:

### Step 1: Identify the Reactants
The reactants in the given reaction are:
- \( H_4S_2O_6 \) (which is known as peroxydisulfuric acid)
- \( H_2O \) (water)

### Step 2: Identify the Products
The products of the reaction are:
- \( H_2SO_3 \) (sulfurous acid)
- \( H_2SO_4 \) (sulfuric acid)

### Step 3: Determine the Nature of the Products
Both \( H_2SO_3 \) and \( H_2SO_4 \) contain oxygen, hydrogen, and sulfur. Therefore, they are classified as oxyacids.

### Step 4: Analyze the Oxidation States
- For \( H_2SO_4 \):
- The oxidation state of sulfur (S) is +6.
- This indicates that it is in a higher oxidation state, which corresponds to sulfuric acid.

- For \( H_2SO_3 \):
- The oxidation state of sulfur (S) is +4.
- This indicates that it is in a lower oxidation state, which corresponds to sulfurous acid.

### Step 5: Conclusion
Since both products are oxyacids and one has a higher oxidation state (sulfuric acid) while the other has a lower oxidation state (sulfurous acid), we conclude that:
- The products are two oxyacids: one with the suffix "-ic" (sulfuric acid) and the other with the suffix "-ous" (sulfurous acid).

Thus, the final answer is that the products are two oxyacids, one with the suffix "-ic" and the other with the suffix "-ous".

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