Q40 / 150 · MHT CET 2026 (13 April Shift 2) · Chemistry
How many moles of hydrogen are liberated when $6$ moles of ethyl alcohol reacts with sodium metal?
- A$2$
- Correct answerB$3$
- C$4$
- D$6$
Solution
The balanced chemical equation for the reaction of ethyl alcohol with sodium metal is:
$2\text{C}_2\text{H}_5\text{OH} + 2\text{Na} \rightarrow 2\text{C}_2\text{H}_5\text{ONa} + \text{H}_2$
From the stoichiometry of the reaction, $2$ moles of ethyl alcohol produce $1$ mole of hydrogen gas.
Therefore, the number of moles of hydrogen gas produced by $6$ moles of ethyl alcohol is:
$\dfrac{1}{2} \times 6 = 3$ moles
Answer: $3$
$2\text{C}_2\text{H}_5\text{OH} + 2\text{Na} \rightarrow 2\text{C}_2\text{H}_5\text{ONa} + \text{H}_2$
From the stoichiometry of the reaction, $2$ moles of ethyl alcohol produce $1$ mole of hydrogen gas.
Therefore, the number of moles of hydrogen gas produced by $6$ moles of ethyl alcohol is:
$\dfrac{1}{2} \times 6 = 3$ moles
Answer: $3$
Hence, the correct answer is option: 'B'.