Question

In the reaction \( 2 \, \text{H}_2 + \text{O}_2 \to 2 \, \text{H}_2\text{O} \), if 4 moles of hydrogen react completely with oxygen, how many moles of water will be produced?

• A. \( 2 \, \text{mol} \)
• B. \( 8 \, \text{mol} \)
• C. \( 4 \, \text{mol} \)
• D. \( 1 \, \text{mol} \)

Hint:

In stoichiometry problems, always refer to the balanced equation to use the mole ratio between reactants and products.

Answer 1

The Correct Option is C

Given reaction:

\( 2H_2 + O_2 \rightarrow 2H_2O \)

Step 1: Use the stoichiometric relationship

The balanced equation tells us that for every 2 moles of \( H_2 \) (hydrogen), 2 moles of \( H_2O \) (water) are produced.

Step 2: Set up the proportion

From the balanced equation: \( 2 \, \text{mol} \, H_2 \rightarrow 2 \, \text{mol} \, H_2O \)

Therefore, if 4 moles of hydrogen (\( H_2 \)) react, the number of moles of water produced will be:

\[ \text{moles of } H_2O = \left( \frac{2 \, \text{mol} \, H_2O}{2 \, \text{mol} \, H_2} \right) \times 4 \, \text{mol} \, H_2 = 4 \, \text{mol} \, H_2O \]

 

✅ Final Answer:

The number of moles of water produced is \( \boxed{4 \, \text{mol}} \)