10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be

Options

A. 1 mol
B. 2mol
C. 3 mol
D. 4 mol

Explanation

To determine the amount of water produced from the reaction of hydrogen and oxygen, we can follow these steps:

### Step 1: Calculate the number of moles of hydrogen (H₂)
The formula to calculate the number of moles is:
\[ \text{Number of moles} = \frac{\text{Given weight}}{\text{Molar mass}} \]
For hydrogen (H₂):
- Given weight = 10 g
- Molar mass of H₂ = 2 g/mol

Calculating the moles of hydrogen:
\[ \text{Number of moles of H₂} = \frac{10 \text{ g}}{2 \text{ g/mol}} = 5 \text{ mol} \]

### Step 2: Calculate the number of moles of oxygen (O₂)
Using the same formula:
For oxygen (O₂):
- Given weight = 64 g
- Molar mass of O₂ = 32 g/mol

Calculating the moles of oxygen:
\[ \text{Number of moles of O₂} = \frac{64 \text{ g}}{32 \text{ g/mol}} = 2 \text{ mol} \]

### Step 3: Determine the limiting reactant
The balanced chemical equation for the reaction is:
\[ 2 \text{H₂} + \text{O₂} \rightarrow 2 \text{H₂O} \]
From the equation, we see that:
- 2 moles of H₂ react with 1 mole of O₂.

Now, we have:
- 5 moles of H₂ available
- 2 moles of O₂ available

To find out how much oxygen is needed to react with 5 moles of hydrogen:
\[ \text{Required moles of O₂} = \frac{5 \text{ mol H₂}}{2} = 2.5 \text{ mol O₂} \]
Since we only have 2 moles of O₂, oxygen is the limiting reactant.

### Step 4: Calculate the amount of water produced
According to the balanced equation:
- 1 mole of O₂ produces 2 moles of H₂O.

Thus, 2 moles of O₂ will produce:
\[ \text{Moles of H₂O} = 2 \text{ mol O₂} \times 2 = 4 \text{ mol H₂O} \]

### Final Answer
The amount of water produced in the reaction is **4 moles**.

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