Prussic acid `+O_2overset("Ag")rarr`
The products of above reaction are

Options

A. `C_2N_2,H_2O`
B. `CO_2,H_2O`
C. `CO,CO_2,H_2O`
D. `CO_2,N_2,H_2O`

Answer

To solve the question regarding the reaction of prussic acid (hydrogen cyanide, HCN) with oxygen (O₂) in the presence of silver (Ag), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in the reaction are:
- Prussic acid (HCN)
- Oxygen (O₂)
- Silver (Ag) as a catalyst

### Step 2: Write the Balanced Reaction
When HCN reacts with O₂ in the presence of Ag, it undergoes oxidation. The silver acts as a catalyst to facilitate the reaction. The balanced equation for the reaction can be represented as:

\[ 2 \text{HCN} + \text{O}_2 \xrightarrow{\text{Ag}} \text{C}_2\text{N}_2 + \text{H}_2\text{O} + \text{Ag}_2\text{O} \]

### Step 3: Identify the Products
From the balanced equation, we can identify the products of the reaction:
- Dimer of hydrogen cyanide (C₂N₂)
- Water (H₂O)
- Silver oxide (Ag₂O)

### Step 4: Finalize the Products
Thus, the final products of the reaction are:
- Dinitrile (C₂N₂)
- Water (H₂O)
- Silver oxide (Ag₂O)

### Conclusion
The products of the reaction between prussic acid and oxygen in the presence of silver are C₂N₂, H₂O, and Ag₂O.