Question

Weight (g) of two moles of the organic compound, which is obtained by heating sodium ethanoate with sodium hydroxide in the presence of calcium oxide is :

• A. 32
• B. 30
• C. 18
• D. 16

Answer 1

The Correct Option is A

To solve this problem, we need to understand the chemical reaction involved in heating sodium ethanoate with sodium hydroxide in the presence of calcium oxide. This reaction is known as the decarboxylation of sodium acetate, which leads to the formation of methane.

The balanced chemical equation for this reaction is:

\(2 \text{ CH}_3\text{COONa} + \text{CaO} + \text{NaOH} \rightarrow \text{CH}_4 + 2 \text{Na}_2\text{CO}_3\)

From the equation, it can be seen that 2 moles of sodium acetate produce 1 mole of methane.

Now, let's find the molecular weight of methane, \(\text{CH}_4\):

• Molecular weight of Carbon (C) = 12 g/mol
• Molecular weight of Hydrogen (H) = 1 g/mol
• Molecular weight of Methane (\(\text{CH}_4\)) = 12 + (4 × 1) = 16 g/mol

The problem asks for the weight of the organic compound produced from 2 moles of sodium acetate, which is 1 mole of methane.

The weight of 2 moles of the organic compound (methane) is:

• \(2 \text{ moles of CH}_4 \times 16 \text{ g/mol} = 32 \text{ g}\)

Therefore, the weight of the organic compound produced is 32 g which matches the correct option.