4.3 g of saturated hydrocarbon $(C_{n} H_{(2 n + 2)})$ is burnt completely and all $C O_{2}$ were absorbed in aqueous $N a O H$ solution. A 300 mL of a 2 M $N a O H$ solution was required for complete absorption of $C O_{2}$ . Hence find the value of n.

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Solution

We know,
$2 N a O H + C O_{2} \to N a_{2} C O_{3} + H_{2} O$
So 2 mol $N a O H$ absorbs 1 mol of $C O_{2}$
Here we have,
300 mL of a 2 M $N a O H$ = 600 mmol of $N a O H$
So, 600 mmol of $N a O H$ will absorb 300 mmol of $C O_{2}$

So, we got 300 mmol of $C O_{2}$ by burning 4.3 g of $C_{n} H_{(2 n + 2)}$
So applying POAC on carbon we get,
$\frac{4.3}{14 n + 2} = \frac{0.3}{n}$
So, $n = 6$

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