`4` moles of `NaBH_(4)` react completely with `I_(2)`.
calculate volume of gaseous products at `STP` from above process.
(Give you answer by dividing `4.48`)

Answer

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation
The reaction of sodium borohydride (NaBH₄) with iodine (I₂) can be represented by the following balanced equation:

\[ 2 \, \text{NaBH}_4 + \text{I}_2 \rightarrow 2 \, \text{NaI} + \text{B}_2\text{H}_6 + \text{H}_2 \]

### Step 2: Identify the gaseous products
From the balanced equation, we can see that the gaseous products are:
- Diborane (B₂H₆)
- Hydrogen gas (H₂)

### Step 3: Determine the moles of gaseous products produced
From the balanced equation, we can see that:
- 2 moles of NaBH₄ produce 1 mole of B₂H₆ and 1 mole of H₂.
- Therefore, 4 moles of NaBH₄ will produce:
- 2 moles of B₂H₆
- 2 moles of H₂

### Step 4: Calculate the total moles of gaseous products
Total moles of gaseous products from 4 moles of NaBH₄:
\[ \text{Total moles} = \text{moles of B}_2\text{H}_6 + \text{moles of H}_2 = 2 + 2 = 4 \text{ moles} \]

### Step 5: Calculate the volume of gaseous products at STP
At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, the volume of 4 moles of gaseous products is:
\[ \text{Volume} = \text{Total moles} \times 22.4 \, \text{L/mole} = 4 \times 22.4 = 89.6 \, \text{liters} \]

### Step 6: Divide the volume by 4.48
Finally, we need to report the answer by dividing the total volume by 4.48:
\[ \text{Final Answer} = \frac{89.6 \, \text{liters}}{4.48} = 20 \, \text{liters} \]

### Summary
The volume of gaseous products at STP from the reaction of 4 moles of NaBH₄ with I₂ is **20 liters**.

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