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Stoichiometric Calculations

4 g of a mixt...

Question

$4$ g of a mixture of dry sodium carbonate and sodium bicarbonate containing $75 %$ of the latter was heated until there was no loss in the weight. Calculate the volume of $C O_{2}$ evolved at STP (in mL).

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Solution

The balanced chemical equation for the thermal decomposition of sodium bicarbonate is as given below:
$2 N a H C O_{3} Δ - \to N a_{2} C O_{3} + H_{2} O + C O_{2}$
Thus, the decomposition of $2$ moles of sodium bicarbonate will produce $1$ mole ( $22.4$ L) of $C O_{2}$ at STP.
$N a_{2} C O_{3} a Δ - \to X$
$N a H C O_{3} i n m i x t u r e = 4 \times \frac{75}{100} = 3 g = 0.0357 m o l$
$C O_{2} f o r m e d = \frac{0.0357}{2} m o l$
$= \frac{0.0357}{2} \times 22.4 L C O_{2} a t S T P$
$= 0.4 L = 400 m L$
Hence, $400$ mL of $C O_{2}$ will be obtained.

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