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Characteristics of Equilibrium Constant

50 g CaCO3 ar...

Question

$50 g C a C O_{3}$ are heated to $1073 K$ in a $5 L$ vessel. What percentage of $C a C O_{3}$ would decompose at equilibrium? The value of $K_{p}$ for the reaction.
$C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g)$ is $1.15 a t m$ at $1073 K$ .

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Solution

Amount of $C a C O_{3} = 50 g$
Molar mass of $C a C O_{3} = 40 + 12 \times 3 \times 16 = 100 g m$
number of mole of $C a C O_{3} = \frac{50}{100} = 0.5 m o l e$
$C a C O_{3} ⇌ C a O + C O_{2} (g)$
$k_{p} = P_{C O_{2}} = 1.15 a t m$
volume = $52$ temp = $1073 k$
$n = \frac{P_{C O_{2}} v}{R T} = \frac{1.15 \times 5}{0.0821 \times 1073} = 0.065$
$%$ of $C a C O_{3}$ decompose = $\frac{0.065}{5} \times 100$
$= 1.3 %$

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